Stoichiometry and Chemical Composition

What is the molecular weight of a compound?

Which of the following represents the correct relationship between grams, moles, and Avogadro's number?

When applying stoichiometry to a balanced chemical reaction, what is the most important information to obtain accurate results?

If 10.8 moles of $SO_3$ are present, what is the mass in grams? (Molar mass of $SO_3$ = 80 g/mol)

How many molecules of $O_2$ are present in 0.470g of oxygen gas? (Molar mass of $O_2$ = 32 g/mol, Avogadro's number = $6.022 × 10^{23}$ molecules/mol)

What is the percentage composition by mass of hydrogen in $H_2O$? (Molar mass of H = 1 g/mol, Molar mass of O = 16 g/mol, Molar mass of $H_2O$ = 18 g/mol)

Consider a compound with the empirical formula $CH_2O$. If its molecular weight is approximately 180 g/mol, what is its molecular formula?

How many grams are needed to obtain 5 moles of $NaOH$? (Molar mass: Na = 23 g/mol, O = 16 g/mol, H = 1 g/mol)

If a compound has an empirical formula of $CH_2$ and a molar mass of 56 g/mol, what is its molecular formula?

Which of the following statements correctly differentiates between empirical and molecular formulas?

A compound is found to contain 60g of carbon, 5g of hydrogen, and 35g of oxygen. What is the empirical formula of this compound?

Propane ($C_3H_8$) undergoes combustion with oxygen to produce carbon dioxide and water. If 44g of propane is combusted, what mass of carbon dioxide ($CO_2$) is produced, assuming complete combustion?

If 50 grams of calcium carbonate ($CaCO_3$) is decomposed, what mass of calcium oxide ($CaO$) will be produced? (CaCO3 = 100g/mol, CaO = 56g/mol)

135g of Aluminum (Al) is reacted with 250g of chlorine gas ($Cl_2$), what mass of aluminum chloride ($AlCl_3$) will be produced? (Al = 27g/mol, Cl2 = 71g/mol, AlCl3=133.5g/mol)

If 40 grams of sodium hydroxide (NaOH) is reacted with 60 grams of hydrochloric acid (HCl), what mass of sodium chloride (NaCl) will be produced (NaOH = 40g/mol, HCl = 36.5g/mol, NaCl=58.5g/mol)

A compound has an empirical formula of $C_2H_2O$ and a molecular weight of 170 g/mol. What is the molecular formula of the compound?

If 10 grams of magnesium (Mg) reacts with excess hydrochloric acid (HCl), what mass of hydrogen gas ($H_2$) will be produced (Mg = 24.3g/mol, H2 = 2g/mol)?

What volume of oxygen at STP can be formed from 100.0g of potassium chlorate, $KClO_3$? ($KClO_3$ = 122g/mol)

What volume of nitrogen gas at STP can be formed from 150.0g of ammonium nitrate, $NH_4NO_3$? ($NH_4NO_3$ = 80g/mol)

If 40.0g of calcium carbonate ($CaCO_3$) reacts completely, what volume of carbon dioxide ($CO_2$) is produced at STP? (MM $CaCO_3$ = 100.1 g/mol; $CaCO_3 + 2HCl → CO_2 + H_2O + CaCl_2$)

15.0g of calcium hypochlorite ($Ca(ClO)_2$) decomposes completely. What volume of chlorine gas ($Cl_2$) is formed at STP? (MM $Ca(ClO)_2$ = 142.98 g/mol; $Ca(ClO)_2 → CaCl_2 + Cl_2$)

How many grams of aluminum must react with sulfuric acid ($H_2SO_4$) to produce 1.25 L of hydrogen gas at STP? (MM Al = 27 g/mol; $2Al + 3H_2SO_4 → Al_2(SO_4)_3 + 3H_2$)

How many grams of magnesium (Mg) are needed to react with excess hydrochloric acid to produce 2.50 L of hydrogen gas at STP? (MM Mg = 24.3 g/mol; $Mg + 2HCl → MgCl_2 + H_2$)

What mass of potassium chlorate ($KClO_3$) is required to produce 4.00 L of oxygen gas at STP? (MM $KClO_3$ = 122 g/mol; $2KClO_3 → 2KCl + 3O_2$)

How many grams of zinc (Zn) are needed to react with excess hydrochloric acid to produce 5.00 L of hydrogen gas at STP? (MM Zn = 65.4 g/mol; $Zn + 2HCl → ZnCl_2 + H_2$)

What mass of sulfuric acid ($H_2SO_4$) is required to produce 10.0 L of hydrogen gas at STP when it reacts with excess zinc? (MM $H_2SO_4$ = 98.1 g/mol; $Zn + H_2SO_4 → ZnSO_4 + H_2$)

What volume of oxygen will react with 150 L of hydrogen to form water vapor according to the following balanced equation? $2H_2 + O_2 → 2H_2O$

If 5.00 L of methane gas reacts completely with oxygen gas to form carbon dioxide and water vapor, what volume of oxygen gas is required, assuming constant temperature and pressure? $CH_4 + 2O_2 → CO_2 + 2H_2O$

What volume of carbon dioxide gas at STP is produced by the complete combustion of 10.0 L of ethane gas? $2C_2H_6 + 7O_2 → 4CO_2 + 6H_2O$

A compound contains 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. What is its empirical formula?

A compound has the empirical formula of $C_3H_4O_3$ and a molar mass of 148 g/mol. What is its molecular formula?

If 22 grams of propane ($C_3H_8$) undergoes complete combustion, what mass of water ($H_2O$) is produced?

When 100 grams of calcium carbonate ($CaCO_3$) decomposes, what mass of carbon dioxide ($CO_2$) is produced?

13.5 g of Al reacts with 20.0 g of $Cl_2$. What mass of $AlCl_3$ will be produced?

If 10.0 g of Mg reacts with 25.0 g of $HCl$, what mass of $H_2$ will be produced?

What volume of oxygen gas at STP can be produced by the decomposition of 100 g of $H_2O_2$?

What volume of hydrogen gas, $H_2$ at STP, is produced when 20 grams of Na reacts with excess water?

What volume of $O_2$ is needed to completely react with 2.0 L of $H_2$ to form water?

What volume of carbon dioxide gas at STP is produced by the complete combustion of 5.0 L of methane gas, $CH_4$?

If 20.0 g of calcium carbonate ($CaCO_3$) reacts with excess hydrochloric acid (HCl), what volume of carbon dioxide ($CO_2$) is produced at STP? (Molar mass of $CaCO_3$ = 100.1 g/mol)

When 30.0 g of calcium hypochlorite ($Ca(ClO)_2$) decomposes, what volume of chlorine gas ($Cl_2$) is formed at STP? (Molar mass of $Ca(ClO)_2$ = 142.98 g/mol)

How many grams of aluminum are required to react with sulfuric acid ($H_2SO_4$) to produce 2.50 L of hydrogen gas at STP? (Molar mass of Al = 27 g/mol)

How many grams of magnesium (Mg) are needed to react with excess hydrochloric acid to produce 5.00 L of hydrogen gas at STP? (Molar mass of Mg = 24.3 g/mol)

What mass of potassium chlorate ($KClO_3$) is required to produce 6.00 L of oxygen gas at STP? (Molar mass of $KClO_3$ = 122 g/mol)

How many grams of zinc are needed to react with excess hydrochloric acid to produce 2.50 L of hydrogen gas at STP? (Molar mass of Zn = 65.4 g/mol)

What mass of sulfuric acid ($H_2SO_4$) is required to produce 5.00 L of hydrogen gas at STP when it reacts with excess zinc? (Molar mass $H_2SO_4$ = 98.1 g/mol)

What volume of oxygen will react with 300 L of hydrogen to form water vapor according to the following balanced equation? $2H_2 + O_2 \rightarrow 2H_2O$

How many liters of oxygen gas are needed to react with 10.0 L of methane gas to form carbon dioxide and water vapor, assuming constant temperature and pressure?

What volume of carbon dioxide gas at STP is produced by the complete combustion of 5.00 L of ethane gas? $2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O$

If you have 2 moles of $H_2SO_4$, how many moles of hydrogen atoms do you have?

Consider a compound with the formula $X_2Y_3$. If the molar mass of X is 20 g/mol and the molar mass of Y is 30 g/mol, what is the molar mass of the compound $X_2Y_3$?

A compound is found to have the following percentage composition by mass: 40% carbon, 6.7% hydrogen, and 53.3% oxygen. Assuming the total mass is 100g, how many moles of Carbon are present?

A compound contains 5.0 g of hydrogen and 40.0 g of oxygen. What is the empirical formula of this compound?

If a sample of gas contains $3.011 10^{23}$ molecules, how many moles of gas are present?

What is the difference between the empirical and molecular formulas of a compound, and why is this distinction important in chemistry?

You have a 50g quantity of each of the following compounds: NaCl, $SO_2$, $C_6H_{12}O_6$. Which sample contains the most moles of the compound?

A newly synthesized compound is found to have a percentage composition of 62.04% C, 10.34% H, and 27.52% O by mass. If its molecular weight is determined to be 116 g/mol, what is the molecular formula of the compound?

Consider the reaction: $2A + 3B \rightarrow C$. If you have 4 moles of A and 4 moles of B, which reactant is the limiting reactant?

Compound X has an empirical formula of $C_3H_4$. If its molar mass is 120 g/mol, what is its molecular formula?

If 2.00 L of hydrogen gas is produced at STP, how many grams of magnesium reacted with excess hydrochloric acid?

How many grams of aluminum are needed to react with sulfuric acid to produce 3.75 L of hydrogen gas at STP?

If 6.00 L of oxygen gas are produced at STP, what mass of potassium chlorate ($KClO_3$) was required?

What volume of carbon dioxide at STP is formed from 80.0g of calcium carbonate ($CaCO_3$)?

If 30.0g of calcium hypochlorite ($Ca(ClO)_2$) decomposes completely, what volume of chlorine gas ($Cl_2$) is formed at STP?

What volume of oxygen is required to react completely with 300 L of hydrogen to form water vapor?

How many liters of oxygen gas are needed to react with 10.0 L of methane gas ($CH_4$) to form carbon dioxide and water vapor (assuming constant temperature and pressure)?

What volume of nitrogen gas is required to react completely with 9.00 L of hydrogen gas to form ammonia gas?

How many liters of oxygen gas are needed to react with 16.0 L of propane gas ($C_3H_8$) to form carbon dioxide and water vapor(assuming constant temperature and pressure)?

What volume of carbon dioxide gas at STP is produced by the complete combustion of 5.00 L of ethane gas ($C_2H_6$)?

A compound contains 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. If its molecular weight is approximately 180 g/mol, what is its molecular formula?

A compound is found to contain 5.5g of carbon and 1.1g of hydrogen. What is the empirical formula of this compound?

If 15 grams of $CaCO_3$ is decomposed, what mass of $CaO$ will be produced, assuming the reaction goes to completion? (Molar mass of $CaCO_3$ = 100 g/mol, Molar mass of $CaO$ = 56 g/mol)

Consider the reaction: $2KClO_3 → 2KCl + 3O_2$. If 25.0g of $KClO_3$ decomposes, what volume of $O_2$ is produced at STP? (Molar mass of $KClO_3$ = 122 g/mol)

For the reaction $N_2 + 3H_2 → 2NH_3$, if 5.0 L of $N_2$ reacts completely with excess $H_2$, what volume of $NH_3$ is produced, assuming constant temperature and pressure?

What mass of hydrogen gas ($H_2$) is produced when 2.43 g of magnesium (Mg) reacts with excess hydrochloric acid (HCl)? (Molar mass of Mg = 24.3 g/mol)

A compound containing only carbon and hydrogen is 80% carbon by mass. What is the empirical formula of this compound?

If 75.0g of ammonium nitrate ($NH_4NO_3$) decomposes, what volume of nitrogen gas ($N_2$) is formed at STP? (Molar mass of $NH_4NO_3$ = 80 g/mol)

What volume of hydrogen gas at STP is produced when 5.0g of magnesium (Mg) reacts with excess hydrochloric acid (HCl)? (Molar mass of Mg = 24.3 g/mol)

If 10.0 g of aluminum (Al) is reacted with 15.0 g of chlorine gas ($Cl_2$), what is the limiting reactant? (Molar mass of Al = 27 g/mol, Molar mass of $Cl_2$ = 71 g/mol)

What is the molar mass of $C_{17}H_{20}N_4S$?

If you have 123.2 g of $Cl_2$, how many moles are present?

How many sodium atoms are present in 2.15 moles of sodium?

How many moles are present in 10 grams of $H_2O$?

How many molecules are present in 56 grams of $CO_2$?

What is the mass percentage of oxygen in $CaCO_3$?

Determine the mass percentage of hydrogen in $C_2H_5OH$.

A compound is composed of 24g of carbon, 4g of hydrogen and 32g of oxygen. What is the empirical formula?

A compound has the empirical formula $C_2H_4O$ and a molecular weight of 88 g/mol. What is the molecular formula of the compound?

Which of the following statements correctly describes the relationship between empirical and molecular formulas?

A compound is found to contain 50% X and 50% Y by mass. The molar mass of X is 10 g/mol and the molar mass of Y is 20 g/mol. What is the empirical formula of the compound?

A compound containing only carbon, hydrogen, and oxygen is found to have 40.0% carbon and 6.7% hydrogen by mass. What is the empirical formula of the compound?

Consider the reaction: $4NH_3 + 5O_2 \rightarrow 4NO + 6H_2O$. If 34 g of $NH_3$ (molar mass = 17 g/mol) reacts with 80 g of $O_2$ (molar mass = 32 g/mol), which reactant is the limiting reactant?

For the reaction $2H_2 + O_2 \rightarrow 2H_2O$, if 4.0 L of $H_2$ and 3.0 L of $O_2$ are reacted at the same temperature and pressure, what volume of $H_2O$ can be produced?

A compound has an empirical formula of $C_2H_5$. If its molar mass is 58 g/mol, what is its molecular formula?

Consider the reaction: $Mg + 2HCl \rightarrow MgCl_2 + H_2$. If 2.4 g of Mg (molar mass = 24 g/mol) reacts with excess HCl, what is the theoretical yield of $H_2$ in grams?

If 10.0 g of calcium carbonate ($CaCO_3$) is decomposed, what volume of carbon dioxide ($CO_2$) is produced at STP?

For the reaction $N_2 + 3H_2 \rightarrow 2NH_3$, if 6.0 L of $H_2$ reacts, what volume of $NH_3$ is produced, assuming constant temperature and pressure?

When 20.0 g of sodium hydroxide (NaOH) reacts with 30.0 g of hydrochloric acid (HCl), what is the limiting reactant?

A compound contains 80% carbon and 20% hydrogen by mass. What is the empirical formula of this compound?

Which of the following correctly describes how to convert from grams to moles?

A compound is found to have the empirical formula $CH_2$. If its molecular weight is 70 g/mol, what is its molecular formula?

What is the mass percentage of carbon in $C_2H_6O$?

A compound contains 40% sulfur and 60% oxygen by mass. What is its empirical formula?

If 3.011 x $10^{23}$ molecules of a substance weigh 30 grams, what is the molar mass of the substance?

How many grams are there in 3.0 moles of $K_2CrO_4$?

A compound has the empirical formula $C_3H_4O$ and a molar mass of 168 g/mol. What is its molecular formula?

What is the total number of atoms present in 1 mole of $Fe_2(SO_4)_3$?

Given a compound with the molecular formula $C_4H_{10}$, what is its percentage composition by mass of carbon?

A gaseous compound is found to consist of 85.7% carbon and 14.3% hydrogen by mass. If it has a molar mass of 42.0 g/mol, what is its molecular formula?

In the reaction $Mg + 2HCl → MgCl_2 + H_2$, how many grams of magnesium are needed to produce 2.50 L of hydrogen gas at STP? (MM Mg = 24.3 g/mol)

Consider the reaction: $2KClO_3 → 2KCl + 3O_2$. What mass of potassium chlorate ($KClO_3$) is required to produce 4.00 L of oxygen gas at STP? (MM $KClO_3$ = 122 g/mol)

For the reaction $Zn + 2HCl → ZnCl_2 + H_2$, how many grams of zinc are needed to react with excess hydrochloric acid to produce 5.00 L of hydrogen gas at STP? (MM Zn = 65.4 g/mol)

Given the reaction $Zn + H_2SO_4 → ZnSO_4 + H_2$, what mass of sulfuric acid ($H_2SO_4$) is required to produce 10.0 L of hydrogen gas at STP when it reacts with excess zinc? (MM $H_2SO_4$ = 98.1 g/mol)

In the reaction $2H_2 + O_2 → 2H_2O$, what volume of oxygen will react with 150 L of hydrogen to form water vapor, assuming the reaction goes to completion at the same temperature and pressure?

For the reaction $CH_4 + 2O_2 → CO_2 + 2H_2O$, how many liters of oxygen gas are needed to react with 5.00 L of methane gas to form carbon dioxide and water vapor at constant temperature and pressure?

Consider the reaction $3H_2 + N_2 → 2NH_3$. What volume of nitrogen gas at STP is required to react completely with 3.00 L of hydrogen gas to form ammonia gas?

In the reaction $C_3H_8 + 5O_2 → 3CO_2 + 4H_2O$, how many liters of oxygen gas are needed to react with 8.00 L of propane gas to form carbon dioxide and water vapor at the same temperature and pressure?

Given the reaction $2C_2H_6 + 7O_2 → 4CO_2 + 6H_2O$, what volume of carbon dioxide gas at STP is produced by the complete combustion of 10.0 L of ethane gas?

What volume of chlorine gas at STP can be formed from 15.0g of calcium hypochlorite, $Ca(ClO)_2$? (MM $Ca(ClO)_2$ = 142.98g/mol; $Ca(ClO)_2 → CaCl_2 + Cl_2$)

A compound contains 40.0 g of nitrogen and 60.0 g of oxygen. What is the empirical formula of this compound?

A compound is found to contain 28.5% carbon, 4.8% hydrogen, and 66.7% oxygen by mass. What is its empirical formula?

If 12.5 grams of calcium carbonate ($CaCO_3$) is decomposed, what mass of calcium oxide ($CaO$) will be produced?

If 10 grams of aluminum (Al) is reacted with 15 grams of chlorine gas ($Cl_2$), what is the limiting reactant?

If 20 grams of sodium hydroxide (NaOH) is reacted with 30 grams of hydrochloric acid (HCl), what mass of sodium chloride (NaCl) will be produced?

If 2.5 grams of magnesium (Mg) reacts with excess hydrochloric acid (HCl), what mass of hydrogen gas ($H_2$) will be produced?

What volume of oxygen at STP can be formed from 25.0g of potassium chlorate, $KClO_3$?

What volume of nitrogen gas at STP can be formed from 37.5g of ammonium nitrate, $NH_4NO_3$?

When determining the molar mass of a compound, which of the following factors must be considered?

What is the relationship between the empirical formula and the molecular formula?

Which of the following represents the correct application of Avogadro's number in stoichiometric calculations?

Considering the percentage composition of a compound, what information does it provide about the compound's elemental makeup?

A compound is found to contain 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. Assuming you have a 100g sample, how many moles of hydrogen are present?

You have two compounds: Compound A has a molecular formula of $C_2H_4O_2$, and Compound B has a molecular formula of $C_6H_{12}O_6$. Which compound has a simpler empirical formula?

If 123.2 g of $Cl_2$ is present, what is the best set up to solve for the number of moles present?

How many grams are present in 0.20 moles of $H_2SO_4$?

How many carbon atoms are present in $4.10 x 10^{24}$ atoms of $C_4H_8$?

In the reaction $Mg + 2HCl \rightarrow MgCl_2 + H_2$, what are the reactants?

What are the products of the reaction $CaCO_3 + 2HCl \rightarrow CO_2 + H_2O + CaCl_2$?

In the reaction $Ca(ClO)_2 \rightarrow CaCl_2 + Cl_2$, what is the role of $Ca(ClO)_2$?

What is the molar mass of NaCl?

According to the balanced equation $2H_2 + O_2 \rightarrow 2H_2O$, what is the ratio of hydrogen to oxygen?

Which formula represents the simplest whole-number ratio of atoms in a compound?

What are the products in the following reaction: $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$?

In the reaction $3H_2 + N_2 \rightarrow 2NH_3$, what is the product?

To convert from moles to mass, which of the following is needed?

What is the molecular formula of a compound?

What are the reactants in the reaction $C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O$?

In the reaction $2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O$, what do $C_2H_6$ and $O_2$ represent?

What is Avogadro's number used for?

What is the percentage composition by mass?

Considering the balanced equation: $Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2$, what is the ratio of Zinc to Sulfuric Acid?

In the balanced equation $2KClO_3 \rightarrow 2KCl + 3O_2$, what does $KClO_3$ represent?

What is the empirical formula of glucose ($C_6H_{12}O_6$)?

If you have 5 moles of NaOH, what conversion road are you taking to find the grams present?

Which of the following statements correctly relates the empirical and molecular formulas?

What is the first step in determining the empirical formula from percentage composition data?

What information is needed to determine the empirical formula of a compound?

What is the first step in determining the empirical formula from percent composition?

What is the role of a balanced chemical equation in stoichiometry?

In a mass-to-mass stoichiometry problem, what is the first conversion?

What is the purpose of identifying the limiting reactant in a chemical reaction?

What is the standard temperature and pressure (STP) value used for gases when calculating volume?

In a mass to volume stoichiometry problem, what volume measurement is typically calculated at STP?

Which of the following statements best describes a limiting reactant?

What conversion factor is used to convert moles of a gas to its volume at STP?

Propane ($C_3H_8$) undergoes combustion with oxygen to produce carbon dioxide and water. What type of stoichiometric problem is this?

What is the purpose of finding the empirical formula of a compound?

If a compound has the molecular formula $C_6H_{12}O_6$, what is its empirical formula?

In stoichiometry, what is the significance of a balanced chemical equation?

What type of stoichiometric problem involves converting grams of reactant to grams of product?

What is stoichiometry?

What is the simplest whole-number ratio of atoms in a compound called?

What is the role of the limiting reactant in a chemical reaction?

What is the standard temperature and pressure (STP) used for gas volume calculations?

Which of the following describes the molecular formula?

In a mass to volume stoichiometry problem, what unit is typically used for volume when using STP conditions?

What conversion factor is used to convert grams to moles?

When balancing a chemical equation, which of the following can be changed?

In percentage composition, what is compared to find the percentage of each element?

The molecular formula of a compound is $C_6H_{12}O_6$. What is its empirical formula?

What quantity is numerically equivalent to one mole of a substance?

If the empirical formula of a compound is $CH_2$ and its molecular mass is 28 g/mol, what is its molecular formula?

According to the reaction $Mg + 2HCl \rightarrow MgCl_2 + H_2$, what are the reactants?

In the reaction $CaCO_3 + 2HCl \rightarrow CO_2 + H_2O + CaCl_2$, what does $CaCO_3$ represent?

What are the products of the reaction $Ca(ClO)_2 \rightarrow CaCl_2 + Cl_2$?

In stoichiometry, what does 'STP' stand for?

What is the role of $H_2SO_4$ in the reaction $2Al + H_2SO_4 \rightarrow Al_2(SO_4)_3 + 3H_2$?

What volume of oxygen is required to react with 150L of hydrogen in the reaction $2H_2 + O_2 \rightarrow 2H_2O$?

In the reaction $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$, if 5.00 L of methane gas ($CH_4$) is used, how many liters of oxygen gas ($O_2$) are needed for complete combustion?

What is the product formed from hydrogen and nitrogen gas, according to the reaction $3H_2 + N_2 \rightarrow 2NH_3$?

In the reaction $C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O$, what are the products?

According to the balanced reaction $2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O$, what is ethane ($C_2H_6$)?

What is the simplest whole-number ratio of atoms in a compound known as?

Which of the following shows the correct components for finding the percentage composition of a compound?

What does the molecular formula of a compound indicate?

What is the molar mass of $SO_2$?

Which value represents Avogadro's number?

What is the empirical formula if a compound has a molecular formula of $C_6H_{12}O_6$?

What is the percentage composition of hydrogen in $H_2O$?

In the reaction $2Al + H_2SO_4 \rightarrow Al_2(SO_4)_3 + 3H_2$, what does Al represent?

What is the chemical formula for hydrochloric acid?

In the reaction $2KClO_3 \rightarrow 2KCl + 3O_2$, what does $O_2$ represent?

What is the chemical symbol for zinc?

In the reaction $Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2$, what is the chemical formula for sulfuric acid?

In the reaction $2H_2 + O_2 \rightarrow 2H_2O$, what does $H_2O$ represent?

In the reaction $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$, what are the products?

What does the empirical formula of a compound represent?

If the empirical formula of a compound is $CH_2$ and its molecular formula is $C_2H_4$, what can you conclude?

In stoichiometry, what is the importance of a balanced chemical equation?

What is the role of molar mass in mass-to-mass stoichiometry problems?

In a mass-to-volume stoichiometry problem, what additional information is needed besides the molar mass?

What does STP stand for in the context of gas stoichiometry?

What is a limiting reactant?

In a chemical reaction, how does the limiting reactant affect the amount of product formed?

What is the simplest whole-number ratio of atoms in a compound, as defined in chemistry?

What is the mass of one mole of a substance called?

Which of the following is the formula for calculating the percentage composition of an element in a compound?

What does Avogadro's number represent?

What is the purpose of stoichiometry?

Which of the following is the correct unit for molar mass?

In the molecular formula, $C_6H_{12}O_6$, what does the '6' in $C_6$ represent?

Which of the following correctly describes the relationship between moles, mass, and molar mass?

What is the empirical formula of a compound with the molecular formula $C_2H_4$?

If the empirical formula of a compound is $CH_2O$ and its molecular formula is $C_6H_{12}O_6$, what number do you multiply the empirical formula by to obtain the molecular formula?

Which of the following is required to determine the molecular formula from the empirical formula?

What is the first step in determining the empirical formula of a compound from its percent composition?

In stoichiometry, what does a 'Mass – Volume' problem involve?

What is the molar mass of propane ($C_3H_8$)?

In a balanced chemical equation, what is the significance of the coefficients in front of each compound?

According to the equation $CaCO_3 + 2HCl \rightarrow CO_2 + H_2O + CaCl_2$, what product is a gas at STP?

What is the standard temperature and pressure (STP) condition used for gas calculations?

In the reaction $2KClO_3 \rightarrow 2KCl + 3O_2$, what is the mole ratio of $KClO_3$ to $O_2$?

In the balanced equation $2Al + 3H_2SO_4 \rightarrow Al_2(SO_4)_3 + 3H_2$, what does $H_2SO_4$ represent?

In the reaction $2KClO_3 \rightarrow 2KCl + 3O_2$, what is being decomposed?

Which of the following statements is true about limiting reactants?

In the reaction $Zn + 2HCl \rightarrow ZnCl_2 + H_2$, which element is present in both the reactant and product?

What formula is used to calculate the number of moles (n) from mass (m) and molar mass (M)?

In the reaction $Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2$, what is being produced?

For the reaction $2H_2 + O_2 \rightarrow 2H_2O$, if you have 2 molecules of $H_2$, how many molecules of $H_2O$ can be produced?

In the reaction $3H_2 + N_2 \rightarrow 2NH_3$, what does $NH_3$ represent?

In the reaction $Mg + 2HCl \rightarrow MgCl_2 + H_2$, what is the mole ratio of magnesium (Mg) to hydrochloric acid (HCl)?

According to the reaction $CaCO_3 + 2HCl \rightarrow CO_2 + H_2O + CaCl_2$, how many moles of hydrochloric acid (HCl) are required to react with one mole of calcium carbonate ($CaCO_3$)?

In the reaction $Ca(ClO)_2 \rightarrow CaCl_2 + Cl_2$, what is the mole ratio between calcium hypochlorite ($Ca(ClO)_2$) and chlorine gas ($Cl_2$)?

What volume of hydrogen gas is produced when one mole of Magnesium reacts with excess hydrochloric acid according to the following reaction: $Mg + 2HCl \rightarrow MgCl_2 + H_2$?

In the reaction $2KClO_3 \rightarrow 2KCl + 3O_2$, how many moles of potassium chlorate ($KClO_3$) are required to produce 3 moles of oxygen gas ($O_2$)?

For the reaction $Zn + 2HCl \rightarrow ZnCl_2 + H_2$, what is the mole ratio of zinc (Zn) to hydrogen gas ($H_2$)?

In the reaction $Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2$, how many moles of sulfuric acid ($H_2SO_4$) are needed to produce one mole of hydrogen gas ($H_2$)?

According to the reaction $2H_2 + O_2 \rightarrow 2H_2O$, if you have 2 moles of hydrogen ($H_2$), how many moles of oxygen ($O_2$) are needed for a complete reaction?

In the reaction $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$, how many liters of oxygen gas ($O_2$) are required to react with 1 liter of methane gas ($CH_4$)?

According to the reaction $3H_2 + N_2 \rightarrow 2NH_3$, how many liters of nitrogen gas ($N_2$) are needed to react completely with 3 liters of hydrogen gas ($H_2$)?

What is the simplest whole-number ratio of atoms in a compound?

If you have 5 moles of NaOH, what information do you need to calculate the mass in grams?

What does the molecular formula of a compound represent?

What is the purpose of determining the empirical formula of a compound?

Which of the following is the correct formula for calculating percentage composition of an element in a compound?

How is the amount of each element in a compound expressed in terms of percentage?

If a compound's empirical formula is $CH_2$ and its molecular formula is $C_2H_4$, what does this indicate?

In stoichiometry, a balanced chemical equation is essential because it directly provides what information?

How do you convert from mass to moles?

What is the first step in solving a mass-mass stoichiometry problem?

Which value is needed to convert grams of $O_2$ to the number of molecules?

In a mass-volume stoichiometry calculation, what conversion is typically needed?

In the empirical formula, the subscripts indicate the:

Which of the following is conserved in a balanced chemical equation?

When using stoichiometry to predict the amount of product formed, what assumption is made about the reaction?

What condition is implied when gas volumes are compared directly in a stoichiometry problem?

How does the presence of a limiting reactant affect the theoretical yield of a reaction?

According to the balanced equation $Mg + 2HCl \rightarrow MgCl_2 + H_2$, what is the mole ratio of magnesium (Mg) to hydrogen gas ($H_2$)?

According to the reaction $Ca(ClO)_2 \rightarrow CaCl_2 + Cl_2$, what is produced when calcium hypochlorite decomposes?

In the balanced equation $2Al + 3H_2SO_4 \rightarrow Al_2(SO_4)_3 + 3H_2$, what is the mole ratio of aluminum (Al) to hydrogen gas ($H_2$)?

What are the products of the reaction between magnesium and hydrochloric acid, as shown by the equation $Mg + 2HCl \rightarrow$?

According to the equation $2KClO_3 \rightarrow 2KCl + 3O_2$, what products are formed when potassium chlorate ($KClO_3$) decomposes?

What information is required to calculate the percentage composition of an element in a compound?

Which of the following shows the correct conversion from mass to moles?

In the reaction $Zn + 2HCl \rightarrow ZnCl_2 + H_2$, what gas is produced?

In the reaction $Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2$, what is the name of the compound with the formula $H_2SO_4$?

Which of the following represent the correct conversion from moles to mass?

Based on the balanced equation $2H_2 + O_2 \rightarrow 2H_2O$, what is the volume ratio of hydrogen to oxygen required for the reaction?

How would you calculate the number of molecules in a given mass of a substance?

In the reaction $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$, what are the products formed when methane ($CH_4$) reacts with oxygen ($O_2$)?

What is the formula for calculating percentage composition of an element in a compound?

In stoichiometry, what is a 'stoichiometry map' used for?

What is the importance of a balanced chemical equation in mass-mass stoichiometry problems?

What is the role of molar mass in mass-volume stoichiometry problems?

What conditions are defined by 'STP' in the context of stoichiometry?

What conversion factor is used to convert moles of a gas to volume (in Liters) at STP?

In a chemical reaction, what is meant by the term 'limiting reactant'?

If you have excess hydrochloric acid (HCl) reacting with magnesium (Mg), what does 'excess' indicate?

Which of the following represents the actual number of atoms of each element in a molecule?

What does the percentage composition of a compound represent?

If the molar mass of $SO_3$ is 80 g/mol, what information is needed to convert 123.2g of $Cl_2$ to moles?

Which conversion factor is used to convert moles to number of molecules?

If a compound has an empirical formula of $CH_2O$ and a molecular formula of $C_6H_{12}O_6$, how many times larger is the molecular formula than the empirical formula?

What is the molar mass of a substance?

What is the value of Avogadro's number?

5 mol $NaOH$ converts to how many grams?

What is the first step in determining the empirical formula of a compound from its elemental masses?

If a compound's empirical formula is $CH_2$ and its molecular weight is 42 g/mol, what is its molecular formula?

In stoichiometry, what does a 'Mass to Mass' problem involve?

What is the molar mass of water ($H_2O$)?

Which of the following is the correct formula for calculating moles?

What is the purpose of balancing chemical equations in stoichiometry?

What is the definition of a limiting reactant in a chemical reaction?

In the reaction $Mg + 2HCl \rightarrow MgCl_2 + H_2$, what is/are the product(s)?

According to the reaction $CaCO_3 + 2HCl \rightarrow CO_2 + H_2O + CaCl_2$, what volume of carbon dioxide is formed per mole of $CaCO_3$ at STP?

In the reaction $Ca(ClO)_2 \rightarrow CaCl_2 + Cl_2$, what is produced when calcium hypochlorite decomposes?

What is the volume of hydrogen gas produced relative to the amount of magnesium reacted in the reaction $Mg + 2HCl \rightarrow MgCl_2 + H_2$?

According to the reaction $Zn + 2HCl \rightarrow ZnCl_2 + H_2$, how many moles of hydrochloric acid are required to react with one mole of zinc?

What is the ratio of zinc to sulfuric acid in the reaction $Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2$?

For the reaction $2H_2 + O_2 \rightarrow 2H_2O$, if you start with 150 L of hydrogen, what volume of oxygen is needed for a complete reaction?

In the reaction $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$, how does the volume of oxygen gas required compare to the volume of methane gas?

In the reaction $3H_2 + N_2 \rightarrow 2NH_3$, what volume of nitrogen gas is needed to react with 3.00 L of hydrogen gas?

What is the first step in determining the percentage composition of an element in a compound?

According to the reaction $Mg + 2HCl \rightarrow MgCl_2 + H_2$, what is produced along with magnesium chloride?

Which of the following is the formula for calculating percentage composition?

Based on the reaction $CaCO_3 + 2HCl \rightarrow CO_2 + H_2O + CaCl_2$, what gas is produced when calcium carbonate reacts with hydrochloric acid?

What is the relationship between molecular and empirical formulas?

What value is Avogadro's number used to convert between?

In the reaction $2Al + 3H_2SO_4 \rightarrow Al_2(SO_4)_3 + 3H_2$, what gas is produced when aluminum reacts with sulfuric acid?

According to the reaction $2KClO_3 \rightarrow 2KCl + 3O_2$, what gas is produced when potassium chlorate decomposes?

What products are formed in the reaction $Zn + 2HCl \rightarrow ZnCl_2 + H_2$?

If you have 56 grams of $CO_2$, what additional information do you need to determine the number of molecules present?

In the reaction $Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2$, what is produced along with zinc sulfate?

According to the reaction $2H_2 + O_2 \rightarrow 2H_2O$, what volume of oxygen is required to react with 150L of hydrogen?

For the reaction $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$, how many liters of oxygen gas are required to react with 5.00 L of methane gas?

Based on the reaction $3H_2 + N_2 \rightarrow 2NH_3$, what volume of nitrogen gas is required to react completely with 3.00 L of hydrogen gas?

What is the first step in solving mass-to-mass stoichiometry problems?

When a problem asks for the 'volume at STP', what does STP refer to?

What conversion factor is used to convert moles to volume at STP?

In a 'mass to volume' stoichiometry problem, what is the final step after finding the moles of the gas?

What is the empirical formula of a compound with the molecular formula $C_6H_{12}O_6$?

For the reaction $2KClO_3 → 2KCl + 3O_2$, what is the mole ratio of $KClO_3$ to $O_2$?

Molar Mass

Gram-Mole (Mole)

Stoichiometry

Stoichiometric Reaction

Mass to Mole Conversion

Mole to Mass Conversion

Mole to Number of Particles

Percentage Composition

Empirical Formula

Molecular Formula

STP Volume

Grams to Liters (STP)

Liters (STP) to Grams

Volume-Volume Stoichiometry

Mg + 2HCl Reaction

CaCO3 + 2HCl Reaction

Ca(ClO)2 Decomposition

KClO3 Decomposition

Zn + 2HCl Reaction

CH4 + 2O2 Reaction

Mass-Mass Problem

Mass-Volume Problem

Limiting Reactant

Excess Reactant

STP

Molar Volume (at STP)

Mass to Volume Stoichiometry

Al + H2SO4 Reaction

Volume to Mass Stoichiometry

Volume to Volume Stoichiometry

2H2 + O2 Reaction

3H2 + N2 Reaction

C3H8 + 5O2 Reaction

Stoichiometry Calculation

Mass-Mass Stoichiometry

Mass-Volume Stoichiometry

Balanced Equation Importance

Molar Mass in Stoichiometry

Molecular Weight

Mass to Mole

Mole to Mass

Moles to Particles

Percent Composition

Finding Empirical Formula

Finding Molecular Formula

Mass-Mass Stoichiometry Problem

Mass-Volume Stoichiometry Problem

STP conditions

Molar Mass of Compound

Avogadro's Number