Chemistry Final Exam Flashcards
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Questions and Answers

A chemical formula for a molecular compound represents the composition of:

  • a compound
  • a molecule (correct)
  • a solution
  • an element

    • How many atoms of fluorine are present in a molecule of carbon tetrafluoride, CF4?

    4

    What is the formula for zinc fluoride?

    ZnF2

    Name the compound Zn3(PO4)2.

    <p>zinc phosphate</p> Signup and view all the answers

    Name the compound KClO3.

    <p>potassium chlorate</p> Signup and view all the answers

    Name the compound Fe(NO3)2.

    <p>iron(II) nitrate</p> Signup and view all the answers

    Name the compound CF4.

    <p>carbon tetrafluoride</p> Signup and view all the answers

    Name the compound N2O3.

    <p>dinitrogen trioxide</p> Signup and view all the answers

    What is the formula for silicon dioxide?

    <p>SiO2</p> Signup and view all the answers

    What is the formula for dinitrogen trioxide?

    <p>N2O3</p> Signup and view all the answers

    What is the sum of the atomic masses of all the atoms in a formula for a compound?

    <p>formula mass</p> Signup and view all the answers

    What is the formula mass of ethyl alcohol, C2H5OH?

    <p>46.08 amu</p> Signup and view all the answers

    What is the formula mass of (NH4)2SO4?

    <p>132.16 amu</p> Signup and view all the answers

    The molar mass of LiF is 25.94 g/mol. How many moles of LiF are present in 10.37 g?

    <p>0.3998 mol</p> Signup and view all the answers

    How many Mg2+ ions are found in 1.00 mol of MgO?

    <p>6.02 X 10^23</p> Signup and view all the answers

    What is the percentage composition of CF4?

    <p>13.6% C, 86.4% F</p> Signup and view all the answers

    A formula that shows the simplest whole-number ratio of the atoms in a compound is the:

    <p>empirical formula</p> Signup and view all the answers

    What is the empirical formula for a compound that is 53.3% O and 46.7% Si?

    <p>SiO2</p> Signup and view all the answers

    A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula for this compound?

    <p>CF4</p> Signup and view all the answers

    A compound contains 64 g of O and 8 g of H. What is the empirical formula for this compound?

    <p>H2O</p> Signup and view all the answers

    What is the empirical formula for a compound that is 36.1% Ca and 63.9% Cl?

    <p>CaCl2</p> Signup and view all the answers

    A compound contains 27.3 g of C and 72.7 g of O. What is the empirical formula for this compound?

    <p>N2O5</p> Signup and view all the answers

    A compound's empirical formula is N2O5. If the formula mass is 108 amu, what is the molecular formula?

    <p>N2O5</p> Signup and view all the answers

    A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?

    <p>N2O5</p> Signup and view all the answers

    What is the small whole number that appears in front of a formula in a chemical equation?

    <p>a coefficient</p> Signup and view all the answers

    A chemical equation is balanced when the:

    <p>same number of each kind of atom appears in the reactants and in the products</p> Signup and view all the answers

    Which of the following is a formula equation for the formation of carbon dioxide from carbon and oxygen?

    <p>C + O2 -&gt; CO2</p> Signup and view all the answers

    In the chemical equation 2Mg(s) + O2(g) -> 2MgO(s), what does Mg represent?

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

    In an equation, the symbol for a substance in water solution is followed by:

    <p>(aq)</p> Signup and view all the answers

    Which coefficients correctly balance the formula equation CaO + H2O -> Ca(OH)2?

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

    What is the balanced equation for the combustion of sulfur?

    <p>S(s) + O2(g) -&gt; SO2(g)</p> Signup and view all the answers

    In what kind of reaction do two or more substances combine to form a new compound?

    <p>synthesis reaction</p> Signup and view all the answers

    In what kind of reaction does a single compound produce two or more simpler substances?

    <p>decomposition reaction</p> Signup and view all the answers

    The equation A + BX -> AX + B is the general equation for a:

    <p>single-displacement reaction</p> Signup and view all the answers

    The reaction represented by the equation 2Mg(s) + O2(g) -> 2MgO(s) is a:

    <p>synthesis reaction</p> Signup and view all the answers

    The reaction represented by the equation Mg(s) + 2HCl(aq) -> H2(g) + MgCl2(aq) is a:

    <p>single-displacement reaction</p> Signup and view all the answers

    The reaction represented by the equation 2HgO(s) -> 2Hg(l) + O2(g) is a(n):

    <p>decomposition reaction</p> Signup and view all the answers

    In the equation 2Al(s) + 3Fe(NO3)2(aq) -> 3Fe(s) + 2Al(NO3)3(aq), iron has been replaced by:

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

    The ability of an element to react is the element's:

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

    An element in the activity series can replace any element:

    <p>below it on the list</p> Signup and view all the answers

    Predict what happens when calcium metal is added to a solution of magnesium chloride.

    <p>calcium chloride</p> Signup and view all the answers

    Predict what happens when nickel is added to a solution of potassium chloride.

    <p>no reaction occurs</p> Signup and view all the answers

    Which of the following would not be studied in the branch of chemistry called stoichiometry?

    <p>the amount of energy required to break the ionic bonds in calcium fluoride</p> Signup and view all the answers

    A balanced chemical equation allows one to determine the:

    <p>mole ratio of any two substances in the reaction</p> Signup and view all the answers

    Each reaction stoichiometry problem requires using a:

    <p>chart of electron configuration</p> Signup and view all the answers

    In the reaction represented by the equation C + 2H2 -> CH4, what is the mole ratio of hydrogen to methane?

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

    In the reaction represented by the equation N2 + 3H2 -> 2NH3, what is the mole ratio of hydrogen to ammonia?

    <p>3:2</p> Signup and view all the answers

    The Haber process for producing ammonia commercially is represented by the equation N2(g) + 3H2(g) -> 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required?

    <p>3.0 mol</p> Signup and view all the answers

    For the reaction represented by the equation 2H2 + O2 -> 2H2O, how many moles of water can be produced from 6.0 mol of oxygen?

    <p>12 mol</p> Signup and view all the answers

    For the reaction represented by the equation 2H2 + O2 -> 2H2O, how many grams of water are produced from 6.00 mol of hydrogen?

    <p>108 g</p> Signup and view all the answers

    For the reaction represented by the equation SO3 + H2O -> H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid in an excess of water?

    <p>320 g</p> Signup and view all the answers

    For the reaction represented by the equation 2HNO3 + Mg(OH)2 -> Mg(NO3)2 + 2H2O, how many grams of magnesium nitrate are produced from 8.00 mol of nitric acid, HNO3, and an excess of Mg(OH)2?

    <p>593 g</p> Signup and view all the answers

    For the reaction represented by the equation Cl2 + 2KBr -> 2KCl + Br2, how many grams of potassium chloride can be produced from 300.g each of chlorine and potassium bromide?

    <p>188 g</p> Signup and view all the answers

    To determine the limiting reactant in a chemical reaction, one must know the:

    <p>available amount of each reactant</p> Signup and view all the answers

    To determine the limiting reactant in a chemical reaction involving known masses of A and B, one could first calculate:

    <p>the number of moles of B and the number of moles of A available</p> Signup and view all the answers

    What is the ratio of the actual yield to the theoretical yield, multiplied by 100%?

    <p>percentage yield</p> Signup and view all the answers

    What is the measured amount of a product obtained from a chemical reaction?

    <p>actual yield</p> Signup and view all the answers

    What is the maximum possible amount of product obtained in a chemical reaction?

    <p>theoretical yield</p> Signup and view all the answers

    A chemist interested in the efficiency of a chemical reaction would calculate the:

    <p>percentage yield</p> Signup and view all the answers

    If the percentage yield is equal to 100%, then:

    <p>the actual yield is equal to the theoretical yield</p> Signup and view all the answers

    For the reaction represented by the equation CH4 + 2O2 -> 2H2O + CO2, calculate the percentage yield of carbon dioxide if Laura Buckley and Andrea Case react 1000.g of methane with excess oxygen and find that they have produced 2300.g of carbon dioxide.

    <p>83.88%</p> Signup and view all the answers

    According to the kinetic-molecular theory, gases condense into liquids because of:

    <p>forces between molecules</p> Signup and view all the answers

    The kinetic-molecular theory explains the behavior of:

    <p>solids, liquids, and gases</p> Signup and view all the answers

    Unlike in an ideal gas, in a real gas:

    <p>the particles exert attractive forces on each other</p> Signup and view all the answers

    According to the kinetic-molecular theory, particles of an ideal gas:

    <p>neither attract nor repel each other but collide</p> Signup and view all the answers

    What determines the average kinetic energy of the molecules of any gas?

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

    Which is an example of effusion?

    <p>air slowly escaping from a pinhole in a tire</p> Signup and view all the answers

    What happens to the volume of a gas during compression?

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

    Study Notes

    Chemical Formulas and Composition

    • Chemical formula denotes the composition of a molecule.
    • Example: In carbon tetrafluoride (CF4), there are 4 fluorine atoms.

    Common Chemical Compounds

    • Zinc fluoride's formula is ZnF2.
    • The compound Zn3(PO4)2 is named zinc phosphate.
    • KClO3 is referred to as potassium chlorate.
    • Fe(NO3)2 is known as iron(II) nitrate.
    • CF4 corresponds to carbon tetrafluoride.
    • N2O3 is named dinitrogen trioxide.
    • The formula for silicon dioxide is SiO2.

    Formula Mass and Molar Mass

    • The term "formula mass" refers to the total atomic mass of all atoms in a compound.
    • Ethyl alcohol (C2H5OH) has a formula mass of 46.08 amu.
    • The formula mass of ammonium sulfate ((NH4)2SO4) is 132.16 amu.
    • Molar mass of LiF is 25.94 g/mol; 10.37 g of LiF corresponds to about 0.3998 mol.

    Empirical Formulas

    • Empirical formulas represent the simplest whole-number ratio of atoms in a compound.
    • The empirical formula for a compound composed of 53.3% O and 46.7% Si is SiO2.
    • For a compound with 259.2 g of F and 40.8 g of C, the empirical formula is CF4.
    • A compound containing 64 g of O and 8 g of H has the empirical formula H2O.
    • The empirical formula for a compound made of 36.1% Ca and 63.9% Cl is CaCl2.

    Chemical Reactions and Balancing Equations

    • A chemical equation is balanced when each type of atom is equal on both sides.
    • In the equation 2Mg(s) + O2(g) → 2MgO(s), Mg is the magnesium reagent.
    • The balanced equation for oxidation of sulfur is S(s) + O2(g) → SO2(g).
    • Synthesis reactions occur when two or more substances create a new compound, while decomposition reactions break down a compound into simpler components.

    Stoichiometry and Moles

    • Stoichiometry involves calculating the mole ratio of substances in a reaction.
    • In the reaction N2 + 3H2 → 2NH3, the mole ratio of hydrogen to ammonia is 3:2.
    • The Haber process requires 3.0 moles of nitrogen gas to completely convert 9.0 moles of hydrogen gas to ammonia.

    Yield and Efficiency in Reactions

    • Actual yield refers to the measured amount of product from a chemical reaction.
    • Theoretical yield indicates the maximum possible product.
    • Percentage yield compares actual yield to theoretical yield expressed as a percentage.
    • A 100% yield indicates actual equals theoretical yield.

    Kinetic-Molecular Theory

    • The kinetic-molecular theory describes the behavior of solids, liquids, and gases.
    • Real gases differ from ideal gases due to intermolecular forces.
    • Changes in temperature directly affect the average kinetic energy of gas molecules.
    • Effusion is exemplified by air escaping from a punctured tire.

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