Q: Calculate the theoretical yield of AgCl (in grams) when 0.30 mol of NaCl reacts with excess AgNO$$_3. ($$Molar mass of AgCl = 143.32 g/mol)

$$0.30 \times 143.32 = 42.996 g$$

Question 1

Which of the following best describes the limiting reactant in a chemical reaction?

Accepted Answer

The reactant that determines the amount of product formed.

Question 2

A student mixes 0.50 mol of AgNO$$_3$$ with 0.30 mol of NaCl. What is the limiting reactant in the reaction: $$\mathrm{$$AgNO_3$$ (aq) + NaCl (aq) \rightarrow AgCl (s) + $$NaNO_3$$ (aq)}$$?

Accepted Answer

NaCl

Question 3

Calculate the theoretical yield of AgCl (in grams) when 0.30 mol of NaCl reacts with excess AgNO$$_3. ($$Molar mass of AgCl = 143.32 g/mol)

Accepted Answer

$$0.30 	imes 143.32 = 42.996 g$$

Question 4

Which of the following equations represents a total ionic reaction for the precipitation of AgCl from AgNO$$_3$$ and NaCl?

Accepted Answer

$$\mathrm{Ag^+ (aq) + NO_3$^- (aq) + Na^+ (aq) + Cl^- (aq) \rightarrow AgCl (s) + Na^+ (aq) + NO_3$^- (aq)}$$

Question 5

If 10.0 g of CaCl$$_2$$ reacts with 12.0 g of Na$$_2CO$_3$$, which is the limiting reactant? (Molar masses: CaCl$$_2 = 110.98 g/$$mol, Na$$_2CO$_3 = 105.99 g/$$mol)

Accepted Answer

Na$$_2CO$_3$$

Question 6

Which of the following is NOT a step in solving a stoichiometry problem?

Accepted Answer

Ignoring the mole ratio between reactants and products

Question 7

A solution contains 0.20 mol of Pb(NO$$_3$$)$$_2$$ and 0.30 mol of KI. What is the maximum number of moles of PbI$$_2$$ that can be formed? $$\mathrm{Pb(NO_3$)_2 (aq) + 2KI (aq) \rightarrow $$PbI_2$$ (s) + 2KNO_3 (aq)}$$

Accepted Answer

0.10 mol

Question 8

Which of the following best describes a net ionic equation?

Accepted Answer

An equation showing only the ions that participate in the reaction.

Question 9

Given the reaction $$\mathrm{$$BaCl_2$$ (aq) + Na_2SO_4 (aq) \rightarrow $$BaSO_4$$ (s) + 2NaCl (aq)}$$, which compound will precipitate?

Accepted Answer

BaSO$$_4$$

Question 10

A hospital uses 250 g of NaCl to prepare a saline solution. How many moles of NaCl are used? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$$\frac{250}{58.44} = 4.28$$ mol

Question 11

Which of the following pairs of ions will NOT form a precipitate when mixed in aqueous solution, according to typical solubility rules?

Accepted Answer

Na$$^+$$ and NO$$_3^-$$

Question 12

A student mixes solutions of K$$_2SO$_4$$ and Pb(NO$$_3$$)$$_2. $$What is the net ionic equation for the formation of the precipitate?

Accepted Answer

$$\mathrm{Pb$$^{2+}$$ (aq) + SO_4$^{2-} (aq) \rightarrow $$PbSO_4$$ (s)}$$

Question 13

Which statement about excess reactant is correct?

Accepted Answer

It remains after the reaction is complete.

Question 14

A chemist combines 0.40 mol of Al and 0.80 mol of O$$_2 to $$produce Al$$_2O$_3. $$What is the theoretical yield of Al$$_2O$_3 in $$moles? $$\mathrm{4Al + 3O_2 \rightarrow 2Al_2O_3}$$

Accepted Answer

0.20 mol

Question 15

Which of the following is a correct molecular equation for the reaction between Na$$_2SO$_4$$ and BaCl$$_2$$?

Accepted Answer

$$\mathrm{Na_2SO_4 (aq) + $$BaCl_2$$ (aq) \rightarrow $$BaSO_4$$ (s) + 2NaCl (aq)}$$

Question 16

A solution contains 0.25 mol of Ca(NO$$_3$$)$$_2$$ and 0.40 mol of Na$$_2SO$_4. $$What is the maximum number of moles of CaSO$$_4$$ that can be formed? $$\mathrm{Ca(NO_3$)_2 (aq) + Na_2SO_4 (aq) \rightarrow $$CaSO_4$$ (s) + 2NaNO_3 (aq)}$$

Accepted Answer

0.25 mol

Question 17

Which of the following is a common misconception about solubility rules?

Accepted Answer

All chlorides are insoluble in water.

Question 18

A patient receives an intravenous solution containing KCl. Which of the following best explains why KCl does not form a precipitate in the bloodstream?

Accepted Answer

K$$^+$$ and Cl$$^-$$ ions are both highly soluble in water.

Question 19

Which of the following is the correct net ionic equation for the reaction between AgNO$$_3$$ and NaCl?

Accepted Answer

$$\mathrm{Ag^+ (aq) + Cl^- (aq) \rightarrow AgCl (s)}$$

General Chemistry: Stoichiometry, Limiting Reactants, Theoretical Yield, and Precipitation Reactions

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