Chemistry Quiz: Molarity, Mass, and Laws
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Questions and Answers

What is the molecular mass of water (H2O)?

  • 16 u
  • 20 u
  • 18 u (correct)
  • 22 u

    • One mole of any substance contains 6.022 x 10^23 particles.

    True

    Calculate the molecular mass of carbon dioxide (CO2).

    44 u

    The molar volume of a gas at STP is ________ L.

    <p>22.4</p> Signup and view all the answers

    Match the following terms with their definitions:

    <p>Molecular Mass = Sum of atomic masses in a molecule Formula Mass = Sum of atomic masses in a formula unit Molar Mass = Mass of one mole of a substance in grams Avogadro's Number = Number of particles in one mole</p> Signup and view all the answers

    What is the formula mass of sodium chloride (NaCl)?

    <p>58.5 u</p> Signup and view all the answers

    52 grams of helium (He) equals 52 moles of helium.

    <p>False</p> Signup and view all the answers

    How many atoms are in 52 moles of helium?

    <p>313.144 x 10^23 atoms</p> Signup and view all the answers

    What is the unit of molality?

    <p>mol/kg</p> Signup and view all the answers

    Molarity changes with temperature, but molality does not.

    <p>True</p> Signup and view all the answers

    Calculate the molarity of NaOH if 4 g is dissolved in 250 mL of solution.

    <p>0.32 M</p> Signup and view all the answers

    The molar mass of sodium acetate (CH3COONa) is ______ g/mol.

    <p>82.0245</p> Signup and view all the answers

    What does the Law of Conservation of Mass state?

    <p>Mass can neither be created nor destroyed.</p> Signup and view all the answers

    The Law of Definite Proportions indicates that a compound can consist of varying proportions of elements.

    <p>False</p> Signup and view all the answers

    How many grams of water are produced from the combustion of 4 g of methane (CH4)?

    <p>18 g</p> Signup and view all the answers

    The limiting reagent is the reactant that is present in excess.

    <p>False</p> Signup and view all the answers

    According to the Law of Multiple Proportions, what is the ratio of masses of oxygen that combine with a fixed mass of hydrogen to form H2O and H2O2?

    <p>1:2</p> Signup and view all the answers

    According to Gay Lussac’s Law of Gaseous Volumes, gases combine in a simple ratio by _____ if they are at the same temperature and pressure.

    <p>volume</p> Signup and view all the answers

    What is the molar mass of copper sulfate (CuSO4)?

    <p>159.5 g/mol</p> Signup and view all the answers

    In the reaction 3g of H2 reacts with 29g of O2 to form __________.

    <p>water</p> Signup and view all the answers

    Match the laws of chemical combinations with their corresponding statements:

    <p>Law of Conservation of Mass = Matter cannot be created or destroyed Law of Definite Proportions = Same elements in same proportion by mass Law of Multiple Proportions = Masses in simple whole number ratios Avogadro's Law = Equal volumes of gases contain equal number of molecules</p> Signup and view all the answers

    Which law states that equal volumes of gases should contain equal number of molecules at the same temperature and pressure?

    <p>Avogadro's Law</p> Signup and view all the answers

    Match the following substances with their corresponding molecular weights:

    <p>CH4 = 16 g/mol O2 = 32 g/mol CO2 = 44 g/mol H2O = 18 g/mol</p> Signup and view all the answers

    The relative atomic mass of an atom is based on the mass of carbon-12 atom.

    <p>True</p> Signup and view all the answers

    What is the maximum amount of copper that can be obtained from 100 g of copper sulfate (CuSO4)?

    <p>39.81 g</p> Signup and view all the answers

    What is the ratio of volumes for hydrogen and oxygen gases as they combine to form water?

    <p>2:1</p> Signup and view all the answers

    One mole of ethane (C2H6) contains six moles of hydrogen atoms.

    <p>True</p> Signup and view all the answers

    How many moles of methane are required to produce 22 g of CO2 after combustion?

    <p>1 mole</p> Signup and view all the answers

    What is the volume occupied by 2 moles of oxygen gas?

    <p>44.8 L</p> Signup and view all the answers

    The empirical formula represents the exact number of atoms present in a molecule.

    <p>False</p> Signup and view all the answers

    Calculate the percentage of oxygen in sodium sulfate (Na2SO4).

    <p>64.5%</p> Signup and view all the answers

    The molar mass of ethanol (C2H5OH) is _____ g/mole.

    <p>46</p> Signup and view all the answers

    Match the following compounds with their empirical formulas:

    <p>Glucose = CH2O Ethene = CH2 Ethane = CH3</p> Signup and view all the answers

    Which gas occupies more volume?

    <p>2 moles of O2</p> Signup and view all the answers

    What is the empirical formula of a compound that contains 4.07% Hydrogen, 24.27% Carbon, and 71.65% Chlorine?

    <p>CH2Cl</p> Signup and view all the answers

    Stoichiometry refers to the qualitative relationship between reactants in a chemical reaction.

    <p>False</p> Signup and view all the answers

    How many moles of H2O are produced from the reaction of 2 moles of H2?

    <p>2 moles</p> Signup and view all the answers

    3 grams of H2 will produce 27 grams of H2O.

    <p>True</p> Signup and view all the answers

    What is the molarity of a solution if you have 10 grams of solute in 2 liters of solution, assuming the molar mass is 50 g/mol?

    <p>0.1 M</p> Signup and view all the answers

    The _______ reagent is completely consumed in a chemical reaction.

    <p>limiting</p> Signup and view all the answers

    If 2 × 10^3 g of N2 reacts with 1 × 10^3 g of H2, which reactant will remain unreacted?

    <p>H2</p> Signup and view all the answers

    A mole fraction can be greater than 1.

    <p>False</p> Signup and view all the answers

    What is the equation to use for calculating the dilution of a solution?

    <p>M1V1 = M2V2</p> Signup and view all the answers

    Study Notes

    Laws of Chemical Combinations

    • Law of Conservation of Mass: Matter/mass cannot be created or destroyed. The mass of reactants equals the mass of products.

    • Law of Definite Proportions: A given compound always contains the same elements in the same proportion by mass.

    • Law of Multiple Proportions: If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in a simple whole number ratio.

    Gay-Lussac's Law of Gaseous Volumes

    • Gases combine, or are produced in a chemical reaction, in simple ratios by volume, provided the gases are at the same temperature and pressure.

    Avogadro's Law

    • Equal volumes of gases, at the same temperature and pressure, contain equal numbers of molecules.

    Relative Atomic Mass

    • The mass of an atom relative to $\frac{1}{12}$th the mass of one carbon-12 atom.

    Atomic Mass Unit (amu)

    • A unit of mass exactly equal to $\frac{1}{12}$th the mass of one carbon-12 atom.

    Molecular Mass

    • The sum of the atomic masses of all the atoms in a molecule.

    Formula Mass

    • The sum of the atomic masses of all the atoms in a formula unit of a compound.

    Mole Concept

    • One mole is the amount of substance containing 6.022 x 1023 particles (atoms, molecules, ions, or formula units).

    • Molar mass: The mass of one mole of a substance in grams.

    Molecular Mass Calculations

    • Calculating the molecular mass of compounds like H2O, CO2, and CH4.

    Number of Atoms Calculations

    • Calculating the number of atoms in a given number of moles of a substance, or in a given mass of an element.

    Molar Volume

    • The volume occupied by 1 mole of gas at standard temperature and pressure (STP) is 22.4 liters.

    Percentage Composition

    • Determining the percentage of each element in a compound.

    Empirical and Molecular Formulas

    • Calculating empirical formulas from percentage composition and molecular formulas from empirical formulas and molar mass.

    Stoichiometry

    • Quantitative relationships between reactants and products in a chemical reaction, using balanced equations to determine masses or volumes involved.

    • Calculating the amount of product formed or reactant consumed in a reaction.

    • Identifying the limiting reagent and the excess reagent in a reaction for complete product formation and determining amount of unreacted substance.

    Solutions

    • Defining mass percent, mole fraction, molarity, and molality as ways to express the concentration of a solution.

    • Calculations involving these concentration units.

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    Chemistry Past Paper PDF - M.E.S Indian School 2024-2025

    Description

    Test your understanding of key concepts in chemistry, including molecular mass, molarity, and the laws of conservation and definite proportions. This quiz covers calculations involving water, carbon dioxide, and sodium chloride, among others. Prepare to demonstrate your knowledge of essential chemical principles.

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