Question 1

A sample of a compound contains 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. What is the empirical formula of this compound?

Accepted Answer

$$\mathrm{CH}_2\mathrm{O}$$

Question 2

Which of the following best describes a strong electrolyte in aqueous solution?

Accepted Answer

A compound that completely dissociates into ions in water

Question 3

When balancing the combustion reaction of propane ($$\mathrm{C}_3\mathrm{H}_8$$), what is the correct coefficient for $$\mathrm{O}_2 in $$the balanced equation?

$$\mathrm{C}_3\mathrm{H}_8 + x\ \mathrm{O}_2 \rightarrow 3\ \mathrm{CO}_2 + 4\ \mathrm{H}_2\mathrm{O}$$

Accepted Answer

$$5$$

Question 4

A solution is prepared by dissolving 0.50 mol of NaCl in enough water to make 1.0 L of solution. What is the molarity of the solution?

Accepted Answer

$$0.50\ \mathrm{M}$$

Question 5

Which of the following reactions is a precipitation reaction?

Accepted Answer

$$\mathrm{AgNO}_3(aq) + \mathrm{NaCl}(aq) \rightarrow \mathrm{AgCl}(s) + \mathrm{NaNO}_3(aq)$$

Question 6

Which of the following statements about limiting reactants is correct?

Accepted Answer

The limiting reactant is completely consumed first in a chemical reaction

Question 7

A 10.0 g sample of calcium carbonate ($$\mathrm{CaCO}_3) is $$heated, producing calcium oxide ($$\mathrm{CaO}) $$and carbon dioxide ($$\mathrm{CO}_2). $$What is the theoretical yield of $$\mathrm{CO}_2 (in $$grams)?

$$\mathrm{CaCO}_3(s) \rightarrow \mathrm{CaO}(s) + \mathrm{CO}_2(g)
($$Molar masses: $$\mathrm{CaCO}_3 = 100\ \mathrm{g/mol}$$, $$\mathrm{CO}_2 = 44\ \mathrm{g/mol})$$

Accepted Answer

$$4.4\ \mathrm{g}$$

Question 8

Which of the following is a correct net ionic equation for the reaction between aqueous solutions of sodium sulfate and barium chloride?

Accepted Answer

$$\mathrm{Ba}^{2+}(aq) + \mathrm{SO}_4$$^{2-}$$(aq) \rightarrow \mathrm{BaSO}_4(s)$$

Question 9

Which of the following compounds is most likely to be insoluble in water?

Accepted Answer

$$\mathrm{AgCl}$$

Question 10

A student mixes 50.0 mL of 0.10 M $$\mathrm{HCl}$$ with 50.0 mL of 0.10 M $$\mathrm{NaOH}. $$What is the final concentration of $$\mathrm{NaCl} in $$the resulting solution?

Accepted Answer

$$0.050\ \mathrm{M}$$

Question 11

Which of the following best describes a redox reaction?

Accepted Answer

A reaction in which electrons are transferred between species

Question 12

Which of the following is the correct balanced equation for the combustion of methane ($$\mathrm{CH}_4$$)?

Accepted Answer

$$\mathrm{CH}_4 + 2\ \mathrm{O}_2 \rightarrow \mathrm{CO}_2 + 2\ \mathrm{H}_2\mathrm{O}$$

Question 13

Which of the following species acts as a Brønsted-Lowry base in aqueous solution?

Accepted Answer

$$\mathrm{H}_2O$$

Question 14

A 25.0 mL sample of 0.200 M $$\mathrm{H}_2SO_4 is $$titrated with 0.100 M $$\mathrm{NaOH}. $$What volume of $$\mathrm{NaOH} is $$required to reach the equivalence point?

$$\mathrm{H}_2SO_4 + 2\ \mathrm{NaOH} \rightarrow \mathrm{Na}_2SO_4 + 2\ \mathrm{H}_2O$$

Accepted Answer

$$50.0\ \mathrm{mL}$$

Question 15

Which of the following is a correct statement about the solubility of ionic compounds in water?

Accepted Answer

All nitrates are soluble in water

Question 16

Which of the following is the correct net ionic equation for the reaction of hydrochloric acid with sodium hydroxide?

Accepted Answer

$$\mathrm{H}^+(aq) + \mathrm{OH}^-(aq) \rightarrow \mathrm{H}_2\mathrm{O}(l)$$

Question 17

Which of the following best explains why sodium metal reacts vigorously with water?

Accepted Answer

Sodium has a low ionization energy and readily loses an electron to form $$\mathrm{Na}^+$$

Question 18

Which of the following is a correct molecular equation for the reaction between aqueous solutions of potassium iodide and lead(II) nitrate?

Accepted Answer

$$2\ \mathrm{KI}(aq) + \mathrm{Pb(NO}_3)_2(aq) \rightarrow 2\ \mathrm{KNO}_3(aq) + \mathrm{PbI}_2(s)$$

Question 19

Which of the following gases is produced when hydrochloric acid reacts with sodium sulfide?

Accepted Answer

$$\mathrm{H}_2S$$

General Chemistry Exam Study Guide: Chemical Reactions, Stoichiometry, and Solution Chemistry

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