9. Calculate the molar mass of a sample with a single molecule weighs $$9.31 \times 10^{-23}$$ g.
(A) 56.1 g/mol
(B) $$6.47 \times 10^{41}$$ g/mol
(C) $$6.02 \times 10^{23}$$ g/mol
(D) $$9.31 \times 10^{-23}$$ g/mol

10. What percentage of nitrogen contained in $$(\text{NH}_4)_2\text{CO}_3$$ by mass? (A) 58.3% (B) 14.6% (C) 29.2% (D) 18.8% 

11. The molar mass of a compound is $100\mathrm{g / mol}$ with the percent composition (by mass) of $\mathrm{C:H:0} = 65.45\% : 5.45\% : 29.09\%$ . Determine the empirical formula and the molecular formula. (A)CHO and $\mathrm{C_6H_6O_6}$ (B) $\mathrm{C_3H_7O}$ and $\mathrm{C_6H_6O_2}$ (C) $\mathrm{C_3HO}$ and $\mathrm{C_6H_2O_2}$ (D) $\mathrm{CH}_2\mathrm{O}$ and $\mathrm{C_4H_8O_4}$

12. There is $100.0\mathrm{g}$ samples of the following compounds: $\mathrm{NH}_3$ , $\mathrm{N}_2\mathrm{O}$ , HCN, $\mathrm{N}_2\mathrm{H}_4$ , and $\mathrm{HNO}_3$ . Which sample has the least mass percent of nitrogen? (A) $\mathrm{NH}_3$ (B) $\mathrm{N}_2\mathrm{O}$ (C)HCN (D) $\mathrm{HNO}_3$

13. How many milliliters of $18.2\mathrm{M}$ $\mathrm{H}_2\mathrm{SO}_4$ are needed to prepare $600.0~\mathrm{mL}$ of $0.10\mathrm{M}$ $\mathrm{H}_2\mathrm{SO}_4$ ? (A) $0.30\mathrm{mL}$ (B) $109\mathrm{mL}$ (C) $3.3\mathrm{mL}$ (D) $1.6\mathrm{mL}$

14. Which of the following concentration measures will change in value as the temperature of a solution changes? (A) mass percent (B) mole fraction (C)molality (D) molarity

15. Consider the reaction $\mathrm{2H_2 + O_2\rightarrow 2H_2O}$ What is the ratio of the initial rate of the appearance of water to the initial rate of disappearance of oxygen? (A)1:1 (B)2:1 (C)1:2 (D)3:2

16. Consider the reaction $\mathrm{X}\rightarrow \mathrm{Y} + \mathrm{Z}$ Which of the following is a possible rate law? (A)Rate=k[X] (B)Rate=k[Y] (C)Rate=k[Y][Z] (D)Rate=k[Z]

17. Which of the following is true about a system at equilibrium? (A) The concentration(s) of the reactant(s) is equal to the concentration(s) of the product(s). (B) No new product molecules are formed. (C) The concentration(s) of reactant(s) is constant over time. (D) The rate of the reverse reaction is equal to the rate of the forward reaction and both rates are equal to zero.

18. For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container. $$ \mathrm {A} (\mathrm {g}) + 2 \mathrm {B} (\mathrm {g}) \rightleftharpoons \mathrm {C} (\mathrm {g}) $$ At equilibrium, the concentration of A is $0.261\mathrm{mol / L}$ . What is the concentration of B at equilibrium? (A)0.261 mol/L (B)0.355 mol/L (C)0.500 mol/L (D)0.522 mol/L

19. For the equilibrium that exists in an aqueous solution of nitrous acid $(\mathrm{HNO}_2$ , a weak acid), the equilibrium constant expression is: (A) \(K = \frac{[\mathrm{H}^{+}][\mathrm{NO}_{2}^{-}]}{[\mathrm{HNO}_{2}]}\) (B) \(K = \frac{[\mathrm{H}^{+}][\mathrm{N}^{2+}][\mathrm{O}^{2-}]^2}{[\mathrm{HNO}_2]}\) (C) \(K = [\mathrm{H}^{+}]\mathrm{[NO}_{2}^{-}]\) (D) \(K = \frac{[\mathrm{H}^{+}]^{2}[\mathrm{NO}_{2}^{-}]}{[\mathrm{HNO}_{2}]}\)

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