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Questions and Answers
If 10 grams of silicon dioxide are heated to decompose it into silicon and oxygen, how much oxygen would be produced, assuming that 46.7% of silicon dioxide is silicon?
If 10 grams of silicon dioxide are heated to decompose it into silicon and oxygen, how much oxygen would be produced, assuming that 46.7% of silicon dioxide is silicon?
- 5.33 grams (correct)
- 5.67 grams
- 4.67 grams
- 10 grams
What mass of sodium chloride (NaCl) would be required to react completely with 34.0g of silver nitrate (AgNO3) to produce 17g of sodium nitrate (NaNO3) and 28.7g of silver chloride (AgCl) based on the Law of Conservation of Mass?
What mass of sodium chloride (NaCl) would be required to react completely with 34.0g of silver nitrate (AgNO3) to produce 17g of sodium nitrate (NaNO3) and 28.7g of silver chloride (AgCl) based on the Law of Conservation of Mass?
- 28.7g
- 34.0g
- 17.0g (correct)
- 51.7g
What is the mass of sodium carbonate produced when 224.4 g of sodium hydroxide reacts with 88 g of carbon dioxide?
What is the mass of sodium carbonate produced when 224.4 g of sodium hydroxide reacts with 88 g of carbon dioxide?
- 276.4g (correct)
- 224.4g
- 36g
- 88g
What is the empirical formula of sucralose if its percentage composition is C= 36.25%, H= 4.82%, Cl= 26.75% and O= 32.19%?
What is the empirical formula of sucralose if its percentage composition is C= 36.25%, H= 4.82%, Cl= 26.75% and O= 32.19%?
How much oxygen is required to produce 0.1618 g of magnesium oxide (MgO) if 0.0976 g of magnesium is heated in the air?
How much oxygen is required to produce 0.1618 g of magnesium oxide (MgO) if 0.0976 g of magnesium is heated in the air?
What is the relative atomic mass of chlorine, given that the abundance of Cl-35 is 75% and that of Cl-37 is 25%?
What is the relative atomic mass of chlorine, given that the abundance of Cl-35 is 75% and that of Cl-37 is 25%?
What is the molecular mass of H2SO4?
What is the molecular mass of H2SO4?
What is the empirical formula of a compound that contains 0.25 moles of carbon and 0.75 moles of hydrogen?
What is the empirical formula of a compound that contains 0.25 moles of carbon and 0.75 moles of hydrogen?
A compound has an empirical formula of CH2 and a molecular mass of 84 gmol-1. What is the molecular formula of this compound?
A compound has an empirical formula of CH2 and a molecular mass of 84 gmol-1. What is the molecular formula of this compound?
Which of the following statements accurately describes the Law of Conservation of Mass?
Which of the following statements accurately describes the Law of Conservation of Mass?
If 10 g of calcium carbonate (CaCO3) decomposes to produce 4.4 g of carbon dioxide (CO2) and 5.6 g of calcium oxide (CaO), which of the following statements is true?
If 10 g of calcium carbonate (CaCO3) decomposes to produce 4.4 g of carbon dioxide (CO2) and 5.6 g of calcium oxide (CaO), which of the following statements is true?
What is the mass of oxygen needed to react completely with 16 grams of methane (CH4) to produce carbon dioxide (CO2) and water (H2O)?
What is the mass of oxygen needed to react completely with 16 grams of methane (CH4) to produce carbon dioxide (CO2) and water (H2O)?
What is the empirical formula of a compound containing 40% carbon, 6.7% hydrogen, and 53.3% oxygen?
What is the empirical formula of a compound containing 40% carbon, 6.7% hydrogen, and 53.3% oxygen?
What is the molecular mass of glucose (C6H12O6)?
What is the molecular mass of glucose (C6H12O6)?
In the following reaction, 2Na + Cl2 → 2NaCl, which of the following is correct?
In the following reaction, 2Na + Cl2 → 2NaCl, which of the following is correct?
Which of the following is not a valid application of the law of conservation of mass?
Which of the following is not a valid application of the law of conservation of mass?
What is the empirical formula of a compound that contains 50% carbon and 50% oxygen by mass?
What is the empirical formula of a compound that contains 50% carbon and 50% oxygen by mass?
A compound has a molecular mass of 180 gmol-1 and an empirical formula of CH2O. What is its molecular formula?
A compound has a molecular mass of 180 gmol-1 and an empirical formula of CH2O. What is its molecular formula?
How many grams of sodium chloride (NaCl) are produced when 11.7 g of sodium (Na) react completely with excess chlorine (Cl2)?
How many grams of sodium chloride (NaCl) are produced when 11.7 g of sodium (Na) react completely with excess chlorine (Cl2)?
Which of the following equations represents the law of conservation of mass in the form commonly used in fluid mechanics and continuum mechanics?
Which of the following equations represents the law of conservation of mass in the form commonly used in fluid mechanics and continuum mechanics?
What is the symbol for the element that has a valency of 2, 4, and 5?
What is the symbol for the element that has a valency of 2, 4, and 5?
What is the correct chemical formula for calcium trioxocarbonate (IV)?
What is the correct chemical formula for calcium trioxocarbonate (IV)?
Which of the following elements has the chemical symbol 'K'?
Which of the following elements has the chemical symbol 'K'?
Which of the following is a characteristic of a compound?
Which of the following is a characteristic of a compound?
What is the valency of chlorine in the compound NaCl?
What is the valency of chlorine in the compound NaCl?
What is the name of the compound with the formula Mg(OH)2?
What is the name of the compound with the formula Mg(OH)2?
What is the relative atomic mass of chlorine if chlorine-35 has an abundance of 75% and chlorine-37 has an abundance of 25%?
What is the relative atomic mass of chlorine if chlorine-35 has an abundance of 75% and chlorine-37 has an abundance of 25%?
What is the correct formula for iron (III) oxide?
What is the correct formula for iron (III) oxide?
Flashcards
Law of Conservation of Mass
Law of Conservation of Mass
Mass of reactants equals mass of products in a chemical reaction.
Reaction of NaOH and CO2
Reaction of NaOH and CO2
When sodium hydroxide reacts with carbon dioxide, sodium carbonate and water are produced.
Percent Composition
Percent Composition
The percentage by mass of each element in a compound.
Differences between Mixtures and Compounds
Differences between Mixtures and Compounds
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Calculating Reactants from Products
Calculating Reactants from Products
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Brezelius' Symbols
Brezelius' Symbols
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Valency
Valency
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Heterogeneous Mixture
Heterogeneous Mixture
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Homogeneous Mixture
Homogeneous Mixture
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Compound
Compound
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Sodium Chloride
Sodium Chloride
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Relative Atomic Mass
Relative Atomic Mass
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Percent Abundance
Percent Abundance
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Calculation of Relative Atomic Mass for Carbon
Calculation of Relative Atomic Mass for Carbon
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Relative Atomic Mass of Chlorine
Relative Atomic Mass of Chlorine
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Empirical Formula
Empirical Formula
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Calculating Empirical Formula from Composition
Calculating Empirical Formula from Composition
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Molecular Formula
Molecular Formula
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Continuity Equation in Fluid Mechanics
Continuity Equation in Fluid Mechanics
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Combustion as Conservation of Mass Example
Combustion as Conservation of Mass Example
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Reaction Mass Conservation Problem
Reaction Mass Conservation Problem
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Calculating Mass with Conservation of Mass
Calculating Mass with Conservation of Mass
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NaOH Molecular Weight Calculation
NaOH Molecular Weight Calculation
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Empirical Formula Calculation Example (MgO)
Empirical Formula Calculation Example (MgO)
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Chemical Reaction Example for Law of Conservation of Mass
Chemical Reaction Example for Law of Conservation of Mass
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Mass Calculation in Reactions
Mass Calculation in Reactions
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Study Notes
Periodic Table Symbols and Names
- Modern chemical symbols, proposed by Berzelius in 1814, use the first letter (capital) or the first and another letter(s) of the element's name (Latin, Greek, or English).
First 30 Elements and Symbols
- Hydrogen (H)
- Helium (He)
- Lithium (Li)
- Beryllium (Be)
- Boron (B)
- Carbon (C)
- Nitrogen (N)
- Oxygen (O)
- Fluorine (F)
- Neon (Ne)
- Sodium (Na)
- Magnesium (Mg)
- Aluminum (Al)
- Silicon (Si)
- Phosphorus (P)
- Sulfur (S)
- Chlorine (Cl)
- Argon (Ar)
- Potassium (K)
- Calcium (Ca)
- Scandium (Sc)
- Titanium (Ti)
- Vanadium (V)
- Chromium (Cr)
- Manganese (Mn)
- Iron (Fe)
- Cobalt (Co)
- Nickel (Ni)
- Copper (Cu)
- Zinc (Zn)
Valencies of Elements
- Valency represents an element's combining power in a chemical reaction.
- It's the number of electrons an element can gain or lose.
- Some elements exhibit multiple valencies (e.g., Fe, Cu, Sn, Pb).
Examples of Elements and Their Valencies
- Hydrogen (H) - Valency 1
- Magnesium (Mg) - Valency 2
- Zinc (Zn) - Valency 2
- Sodium (Na) - Valency 1
- Calcium (Ca) - Valency 2
- Lead (Pb) - Valency 2, 4
- Chlorine (Cl) - Valency -1
- Aluminum (Al) - Valency 3
- Oxygen (O) - Valency -2
- Manganese (Mn) - Valency 2, 4, 5, 7
- Tin (Sn) - Valency 2, 4
- Copper (Cu) - Valency 1, 2
Compound Names and Formulas
- Examples of compound names, chemical formulas, and their constituent elements are provided in the text.
Mixtures vs. Compounds
- Mixtures: Can be homogeneous or heterogeneous; constituents are physically combined in variable ratios; properties are the sum of individual constituents.
- Compounds: Always homogeneous; constituents are chemically combined in fixed ratios; properties are different from those of individual constituents.
Relative Atomic Mass Calculation
- Calculations are shown for determining relative atomic mass from isotopic abundance.
Percentage Composition in Compounds
- Calculations are shown for determining the percentage composition by mass of elements in compounds (e.g., NaOH, H₂SO₄, Ca(OH)₂).
Empirical and Molecular Formulas
- Empirical formula: Shows the simplest whole-number ratio of atoms in a compound (e.g., CH₃).
- Molecular formula: Shows the actual number of atoms of each element in a compound.
- Calculations are provided to determine empirical and molecular formulas from percent compositions and molar masses.
Law of Conservation of Mass
- The law states that mass cannot be created or destroyed in an isolated system; it can only be transformed.
- Mass of reactants = Mass of products in low-energy thermodynamic processes.
- The law has been refined with quantum mechanics and special relativity.
- The law is expressed mathematically using the continuity equation (differential form) in fluid and continuum mechanics.
Law of Conservation of Mass Examples and Calculations
- Examples and calculations provided demonstrate how to calculate unknown masses of reactants or products in chemical reactions while adhering to the law of conservation of mass.
Evaluation and Classwork Questions
- The text provides practice problems to apply concepts related to chemical formulas, valencies, stoichiometry, and the law of conservation of mass.
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