Question 1

A chemist reacts 12.0 g of sodium chloride ($$\mathrm{NaCl}) $$with excess silver nitrate ($$\mathrm{$$AgNO_3$$}) to $$produce silver chloride ($$\mathrm{AgCl}) as a $$precipitate. What mass of $$\mathrm{AgCl}$$ will be formed? (Molar masses: $$\mathrm{NaCl} = 58.44 g/$$mol, $$\mathrm{AgCl} = 143.32 g/$$mol)

Accepted Answer

$$\boxed{29.4\ \mathrm{g}}$$

Question 2

What is the molarity of a solution prepared by dissolving 10.0 g of potassium nitrate ($$\mathrm{$$KNO_3$$}$$, molar mass = 101.1 g/mol) in enough water to make 250 mL of solution?

Accepted Answer

$$\boxed{0.396\ \mathrm{M}}$$

Question 3

Which of the following compounds is a strong electrolyte when dissolved in water?

Accepted Answer

$$\boxed{\mathrm{$$KNO_3$$}}$$

Question 4

A student mixes 100.0 mL of 0.200 M $$\mathrm{$$BaCl_2$$}$$ with 100.0 mL of 0.200 M $$\mathrm{Na_2SO_4}. $$What mass of $$\mathrm{$$BaSO_4$$}$$ precipitate will form? (Molar mass $$\mathrm{$$BaSO_4$$} = 233.4 g/$$mol)

Accepted Answer

$$\boxed{4.67\ \mathrm{g}}$$

Question 5

Which is the correct balanced half-reaction for the reduction of $$\mathrm{$$MnO_4$$^-} to$$ $$\mathrm{Mn$$^{2+}$$} in $$acidic solution?

Accepted Answer

$$\boxed{\mathrm{$$MnO_4$$^-} + 8H^+ + 5e^- \rightarrow Mn$$^{2+}$$ + 4H_2O}$$

Question 6

Which of the following reactions is a redox reaction?

Accepted Answer

$$\boxed{\mathrm{2Na + Cl_2$ \rightarrow 2NaCl}}$$

Question 7

A solution contains 0.50 M $$\mathrm{Ca$$^{2+}$$}$$ and 0.50 M $$\mathrm{Cl^-}. If $$sodium sulfate ($$\mathrm{Na_2SO_4}) is $$added, which compound will precipitate first?

Accepted Answer

$$\boxed{\mathrm{$$CaSO_4$$}}$$

Question 8

Which of the following is the correct net ionic equation for the reaction between hydrochloric acid ($$\mathrm{HCl}) $$and sodium hydroxide ($$\mathrm{NaOH}$$)?

Accepted Answer

$$\boxed{\mathrm{H^+ + OH^- \rightarrow H_2O}}$$

Question 9

A reaction uses 5.00 g of $$\mathrm{Fe}$$ and 8.00 g of $$\mathrm{Cl_2$} to $$produce $$\mathrm{$$FeCl_3$$}. $$Which is the limiting reactant? (Molar masses: $$\mathrm{Fe} = 55.85 g/$$mol, $$\mathrm{Cl_2$} = 70.90 g/$$mol)

Accepted Answer

$$\boxed{\mathrm{Fe}}$$

Question 10

A 50.0 g sample of water is heated from 25.0 $$^\circC to 75.0$$ $$^\circC. $$How much heat ($$q) is $$absorbed? ($$c = 4.18\ \mathrm{J/g\cdot K})$$

Accepted Answer

$$\boxed{10,450\ \mathrm{J}}$$

Question 11

Which set of oxidation numbers is correct for the atoms in $$\mathrm{H_2SO_4}$$?

Accepted Answer

$$\boxed{\mathrm{H = +1, S = +6, O = -2}}$$

Question 12

Given the following reactions and their enthalpy changes:

$$\mathrm{C + O_2$ \rightarrow CO_2$}\quad \Delta H = -393.5\ \mathrm{kJ}$$

$$\mathrm{CO + \frac{1}{2}O_2$ \rightarrow CO_2$}\quad \Delta H = -283.0\ \mathrm{kJ}$$

Calculate $$\Delta H$$ for $$\mathrm{C + \frac{1}{2}O_2$ \rightarrow CO}.$$

Accepted Answer

$$\boxed{-110.5\ \mathrm{kJ}}$$

Question 13

Which of the following is the empirical formula for a compound with 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?

Accepted Answer

$$\boxed{\mathrm{CH_2O}}$$

Question 14

A 0.100 M solution of $$\mathrm{Na_2SO_4} is $$mixed with a 0.100 M solution of $$\mathrm{$$CaCl_2$$}. $$What is the net ionic equation for the precipitation reaction?

Accepted Answer

$$\boxed{\mathrm{Ca$$^{2+}$$ + SO_4$^{2-} \rightarrow $$CaSO_4$$\ (s)}}$$

Question 15

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

Accepted Answer

$$\boxed{25.0\ \mathrm{mL}}$$

Question 16

Which of the following is the correct molecular equation for the reaction between $$\mathrm{H_2SO_4}$$ and $$\mathrm{NaOH}$$?

Accepted Answer

$$\boxed{\mathrm{H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O}}$$

Question 17

A 250 mL solution contains 0.50 M $$\mathrm{Na_2CO_3}. $$How many grams of $$\mathrm{Na_2CO_3}$$ are present? (Molar mass = 106.0 g/mol)

Accepted Answer

$$\boxed{13.25\ \mathrm{g}}$$

Question 18

A reaction produces 15.0 g of $$\mathrm{CO_2$}$$, but the theoretical yield is 20.0 g. What is the percent yield?

Accepted Answer

$$\boxed{75\%}$$

Question 19

A compound has an empirical formula of $$\mathrm{CH_2$}$$ and a molar mass of 56.0 g/mol. What is its molecular formula?

Accepted Answer

$$\boxed{C_4H_8}$$

General Chemistry I: Core Topics and Study Guide

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