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Questions and Answers
How many moles of potassium chlorate (KClO3) are required to produce 1.5 moles of oxygen gas (O2) in the reaction: 2KClO3(s) → 2KCl(s) + 3O2(g)?
How many moles of potassium chlorate (KClO3) are required to produce 1.5 moles of oxygen gas (O2) in the reaction: 2KClO3(s) → 2KCl(s) + 3O2(g)?
In the reaction 4P(s) + 5O2(g) → P4O10(s), what mass of phosphorus (P) is needed to react completely with 10.0 grams of oxygen (O2)?
In the reaction 4P(s) + 5O2(g) → P4O10(s), what mass of phosphorus (P) is needed to react completely with 10.0 grams of oxygen (O2)?
In the decomposition of hydrogen peroxide (2H2O2(aq) → 2H2O(l) + O2(g)), if 5.0 grams of hydrogen peroxide decomposes, what mass of oxygen is produced?
In the decomposition of hydrogen peroxide (2H2O2(aq) → 2H2O(l) + O2(g)), if 5.0 grams of hydrogen peroxide decomposes, what mass of oxygen is produced?
What is the mole ratio between potassium chlorate (KClO3) and potassium chloride (KCl) in the reaction 2KClO3(s) → 2KCl(s) + 3O2(g)?
What is the mole ratio between potassium chlorate (KClO3) and potassium chloride (KCl) in the reaction 2KClO3(s) → 2KCl(s) + 3O2(g)?
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In the reaction 4P(s) + 5O2(g) → P4O10(s), what mass of P4O10 is produced when 5.00 g of phosphorus (P) reacts completely with excess oxygen?
In the reaction 4P(s) + 5O2(g) → P4O10(s), what mass of P4O10 is produced when 5.00 g of phosphorus (P) reacts completely with excess oxygen?
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If 2.50 mol of H2O2 decomposes according to the reaction 2H2O2(aq) → 2H2O(l) + O2(g), how many grams of oxygen gas (O2) will be produced?
If 2.50 mol of H2O2 decomposes according to the reaction 2H2O2(aq) → 2H2O(l) + O2(g), how many grams of oxygen gas (O2) will be produced?
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What mass of phosphorus (P) is required to react completely with 10.0 g of oxygen (O2) in the reaction 4P(s) + 5O2(g) → P4O10(s)?
What mass of phosphorus (P) is required to react completely with 10.0 g of oxygen (O2) in the reaction 4P(s) + 5O2(g) → P4O10(s)?
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In the reaction 2H2O2(aq) → 2H2O(l) + O2(g), how many moles of oxygen (O2) are produced when 1.00 mol of hydrogen peroxide (H2O2) decomposes?
In the reaction 2H2O2(aq) → 2H2O(l) + O2(g), how many moles of oxygen (O2) are produced when 1.00 mol of hydrogen peroxide (H2O2) decomposes?
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In the reaction N2(g) + 3H2(g) → 2NH3(g), how many moles of NH3 are produced when 7.5 moles of H2 react completely?
In the reaction N2(g) + 3H2(g) → 2NH3(g), how many moles of NH3 are produced when 7.5 moles of H2 react completely?
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Which of the following is NOT a step involved in solving stoichiometry problems based on the provided text?
Which of the following is NOT a step involved in solving stoichiometry problems based on the provided text?
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What is the primary purpose of the 'data table' used in the problem-solving example?
What is the primary purpose of the 'data table' used in the problem-solving example?
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In practice problem 1, how many moles of sodium (Na) are required to produce 4.0 moles of hydrogen (H2)?
In practice problem 1, how many moles of sodium (Na) are required to produce 4.0 moles of hydrogen (H2)?
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In the reaction 2Al(s) + 3H2SO4(l) → Al2(SO4)3(aq) + 3H2(g), how many moles of H2SO4 are needed to react completely with 12 mol of Al?
In the reaction 2Al(s) + 3H2SO4(l) → Al2(SO4)3(aq) + 3H2(g), how many moles of H2SO4 are needed to react completely with 12 mol of Al?
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In the reaction 2LiBr(aq) + Cl2(g) → 2LiCl(aq) + Br2(l), if 0.046 mol of LiBr reacts completely, how many moles of LiCl are formed?
In the reaction 2LiBr(aq) + Cl2(g) → 2LiCl(aq) + Br2(l), if 0.046 mol of LiBr reacts completely, how many moles of LiCl are formed?
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What is the mass of water produced by burning 500.g of methane, given the following reaction:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
What is the mass of water produced by burning 500.g of methane, given the following reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
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In Sample Problem 3, the molar mass of Al2O3 was used to convert from grams of Al2O3 to moles of Al2O3. What is the numerical value of this molar mass?
In Sample Problem 3, the molar mass of Al2O3 was used to convert from grams of Al2O3 to moles of Al2O3. What is the numerical value of this molar mass?
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What concept is central to the calculation of the amount of product formed in a chemical reaction, as demonstrated in the example problems?
What concept is central to the calculation of the amount of product formed in a chemical reaction, as demonstrated in the example problems?
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In Sample Problem 3, what is the mole ratio used to convert moles of Al2O3 to moles of Al?
In Sample Problem 3, what is the mole ratio used to convert moles of Al2O3 to moles of Al?
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The step "Multiply by the mole ratio of NH3 to H2 determined from the coefficients of the balanced equation." in the PLAN section relates most directly to which of these concepts?
The step "Multiply by the mole ratio of NH3 to H2 determined from the coefficients of the balanced equation." in the PLAN section relates most directly to which of these concepts?
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In the Practice problem 1, what is the molar mass of Na2CO3 used to calculate the moles of Na2CO3?
In the Practice problem 1, what is the molar mass of Na2CO3 used to calculate the moles of Na2CO3?
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What is the balanced chemical equation for the reaction of sodium carbonate with nitric acid, as shown in Practice problem 1?
What is the balanced chemical equation for the reaction of sodium carbonate with nitric acid, as shown in Practice problem 1?
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In the Practice problem 2, what is the mole ratio of hydrogen to iron in the balanced equation for the production of hydrogen gas?
In the Practice problem 2, what is the mole ratio of hydrogen to iron in the balanced equation for the production of hydrogen gas?
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What is the molar mass of the product, Fe3O4, in the Practice problem 2 equation?
What is the molar mass of the product, Fe3O4, in the Practice problem 2 equation?
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In Sample Problem 4, how many moles of methane are present in 500. g of methane?
In Sample Problem 4, how many moles of methane are present in 500. g of methane?
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What is the mole ratio between CH4 and H2O in the balanced chemical equation for the combustion of methane?
What is the mole ratio between CH4 and H2O in the balanced chemical equation for the combustion of methane?
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In the calculation of the mass of H2O produced, why is the molar mass of CH4 used?
In the calculation of the mass of H2O produced, why is the molar mass of CH4 used?
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If the mass of CH4 used was doubled, what would happen to the mass of H2O produced?
If the mass of CH4 used was doubled, what would happen to the mass of H2O produced?
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What is the mass of silver bromide produced from 50.0 g of silver nitrate using the reaction: 2AgNO3(aq) + MgBr2(aq) → 2AgBr(s) + Mg(NO3)2(aq)?
What is the mass of silver bromide produced from 50.0 g of silver nitrate using the reaction: 2AgNO3(aq) + MgBr2(aq) → 2AgBr(s) + Mg(NO3)2(aq)?
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What is the mass of calcium carbide (CaC2) needed to produce 100 g of acetylene (C2H2) using the reaction: CaC2(s) + 2H2O(l) → C2H2(g) + Ca(OH)2(s)?
What is the mass of calcium carbide (CaC2) needed to produce 100 g of acetylene (C2H2) using the reaction: CaC2(s) + 2H2O(l) → C2H2(g) + Ca(OH)2(s)?
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Which of the following is NOT a step involved in calculating the mass of a product in a chemical reaction?
Which of the following is NOT a step involved in calculating the mass of a product in a chemical reaction?
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Why is the concept of mole ratio important in stoichiometry?
Why is the concept of mole ratio important in stoichiometry?
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How many grams of chlorine gas (Cl2) are produced from the reaction of 25.0 g of MnO2 using the reaction: MnO2(s) + 4HCl(aq) → MnCl2(aq) + 2H2O(l) + Cl2(g)?
How many grams of chlorine gas (Cl2) are produced from the reaction of 25.0 g of MnO2 using the reaction: MnO2(s) + 4HCl(aq) → MnCl2(aq) + 2H2O(l) + Cl2(g)?
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Which of the following is the BEST definition of stoichiometry?
Which of the following is the BEST definition of stoichiometry?
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In the sandwich recipe analogy, what is the mole ratio of bread slices to turkey slices in the recipe?
In the sandwich recipe analogy, what is the mole ratio of bread slices to turkey slices in the recipe?
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What is the coefficient of ZnO in the balanced chemical equation for the reaction of zinc with oxygen? (2Zn + O2 → 2ZnO)
What is the coefficient of ZnO in the balanced chemical equation for the reaction of zinc with oxygen? (2Zn + O2 → 2ZnO)
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According to the balanced chemical equation 2Zn + O2 → 2ZnO, how many moles of ZnO can be produced from 5 moles of Zn?
According to the balanced chemical equation 2Zn + O2 → 2ZnO, how many moles of ZnO can be produced from 5 moles of Zn?
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Which of the following is NOT a step involved in solving stoichiometry problems?
Which of the following is NOT a step involved in solving stoichiometry problems?
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What is the molar mass of zinc oxide (ZnO)?
What is the molar mass of zinc oxide (ZnO)?
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In the reaction 2Zn + O2 → 2ZnO, if you have 10 grams of zinc, how many grams of zinc oxide (ZnO) can you theoretically produce?
In the reaction 2Zn + O2 → 2ZnO, if you have 10 grams of zinc, how many grams of zinc oxide (ZnO) can you theoretically produce?
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Which of the following is a limiting reactant?
Which of the following is a limiting reactant?
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Flashcards
Molar Mass
Molar Mass
The mass of one mole of a substance, usually in grams.
Stoichiometry
Stoichiometry
The calculation of reactants and products in chemical reactions.
Mole Ratio
Mole Ratio
A ratio derived from the coefficients of a balanced equation, used to convert between moles of different substances.
Balanced Equation
Balanced Equation
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Significant Figures
Significant Figures
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Mass of Substance B
Mass of Substance B
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Reactants
Reactants
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Products
Products
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Balanced Chemical Equation
Balanced Chemical Equation
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Chemical Reaction
Chemical Reaction
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Conversion of Mass
Conversion of Mass
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Conversion Factor
Conversion Factor
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Mass Calculation for H2O
Mass Calculation for H2O
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Grams to Moles Conversion
Grams to Moles Conversion
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Propane Combustion Reaction
Propane Combustion Reaction
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Moles of CO2 from Propane
Moles of CO2 from Propane
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Moles of H2O from Propane
Moles of H2O from Propane
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O2 Consumption in Propane Combustion
O2 Consumption in Propane Combustion
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Moles of C3H8 Consumed
Moles of C3H8 Consumed
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Potassium Chlorate Reaction
Potassium Chlorate Reaction
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Mass of KClO3 for O2 Production
Mass of KClO3 for O2 Production
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Conversion from Moles to Mass
Conversion from Moles to Mass
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Molar mass of Al2O3
Molar mass of Al2O3
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Mole ratio in reactions
Mole ratio in reactions
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Calculating moles from mass
Calculating moles from mass
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Conversion factor in chemistry
Conversion factor in chemistry
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Combustion of methane
Combustion of methane
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Water produced in reactions
Water produced in reactions
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Kilograms to grams conversion
Kilograms to grams conversion
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Study Notes
Stoichiometry
- Stoichiometry is the process of relating amounts of reactants and products in a chemical reaction to one another.
- Chemists use chemical equations to make predictions about quantities of substances reacting or being produced.
- Stoichiometry uses mole ratios to calculate quantities.
- Using an analogy of making sandwiches, the recipe demonstrates how ingredients (reactants) relate to a product (sandwich).
- Zinc reacts with oxygen to produce zinc oxide, according to the equation 2Zn + O2 → 2ZnO.
- This equation illustrates the relationship between reactants and products in a chemical reaction.
General Plan for Solving Stoichiometry Problems
- A general plan for solving stoichiometry problems is presented.
- This involves using molar mass conversions to determine amounts in moles.
- The mole ratio from the balanced chemical equation is used to convert between moles of reactants and products.
- Finally, molar mass conversions are used to convert the amount (in moles of substance B) to mass.
Sample Problem 1
- Ammonia is produced by reacting nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g).
- If 4.0 mol of H2 react, the amount of NH3 produced is calculated by multiplying by the mole ratio (2 mol NH3/3 mol H2) which yields 2.7 mol NH3.
Sample Problem 2
- Potassium chlorate decomposes to generate oxygen: 2KClO3(s) → 2KCl(s) + 3O2(g).
- To produce 0.50 mol of O2, the mass of KClO3 needed is calculated by using mole ratios and molar masses from the balanced equation.
- The result is 41 g of KClO3 for 0.50 mol of O2.
Sample Problem 3
- Aluminum reacts with sulfuric acid: 2Al(s) + 3H2SO4(l) → Al2(SO4)3(aq) + 3H2(g).
- The calculation of moles of aluminum produced from 30 kg of Al2O3 is determined by using molar masses and mole ratios. Calculating moles of Al produced from 30 kg Al2O3 is 588 mol Al.
Sample Problem 4
- Methane burns in air: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g).
- The mass of water produced by burning 500 g of methane is calculated by using the equations and molar masses.
- 500 g of methane produces 1120g of H2O.
Practice Problems
- Various practice problems about reactions: calculating moles, masses and ratios of involved reactants and products are provided.
- Including the calculations for Sodium carbonate, Hydrogen, Phosphorus, and more.
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Description
This quiz covers the fundamentals of stoichiometry, the process that relates reactants and products in chemical reactions. You'll learn how to use mole ratios and molar mass conversions to solve stoichiometry problems effectively. The quiz will help reinforce your understanding of chemical equations and their applications.
