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$_2$CO$_3$, which is the limiting reactant? (Molar masses: CaCl$_2$ = 110.98 g/mol, Na$_2$CO$_3$ = 105.99 g/mol)

Accepted Answer

Na$_2$CO$_3$

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$_2$SO$_4$ 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$_2$O$_3$. What is the theoretical yield of Al$_2$O$_3$ 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$_2$SO$_4$ 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$_2$SO$_4$. 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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