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# 14.5: Multimedia Resources for Chapter 14

Difficulty Level: At Grade Created by: CK-12

Copy and distribute the lesson worksheets. Ask students to complete the worksheets alone or in pairs as a review of lesson content.

## Stoichiometry Worksheet

CK-12 Foundation Chemistry

Name______________________ Date_________

1. How many moles are present in $58.6 \ grams$ of lead (II) oxide?

A. $0.113 \ moles$

B. $0.158 \ moles$

C. $0.263 \ moles$

D. $0.300 \ moles$

E. None of these.

2. According to the following balanced equation, how many moles of oxygen can be produced by the complete reaction of $10.0 \ moles$ of potassium chlorate, $KClO_3$?

$2 \ KClO_3 \rightarrow 2\ KCl + 3 \ O_2$

A. $10.0 \ moles$

B. $6.67 \ moles$

C. $15.0 \ moles$

D. $4.00 \ moles$

E. None of these.

3. Balance the following equation and determine how many moles of water will be produced by the complete reaction of $0.600 \ moles$ of aluminum hydroxide?

$\line(1,0){15} \ Al(OH)_3 ~ +~ \line(1,0){15} \ H_2SO_4 \rightarrow~ \line(1,0){15} \ Al_2(SO_4)_3 ~+~ \line(1,0){15} \ H_2O$

A. $1.80 \ moles$

B. $0.200 \ moles$

C. $20.0 \ moles$

D. $0.600 \ moles$

E. None of these.

4. Using the balanced equation, $2 \ KClO_3 \rightarrow 2 \ KCl + 3 \ O_2$, how many moles of $O_2$ can be produced by the complete reaction of $100. \ grams$ of $KClO_3$?

A. $0.326 \ moles$

B. $0.544 \ moles$

C. $0.816 \ moles$

D. $1.22 \ moles$

E. None of these.

5. If hydrogen is completely reacted with oxygen and produces $180. \ grams$ of water, how many grams of hydrogen was consumed? The following equation for the reaction is not yet balanced.

$\line(1,0){15} \ H_2 ~+~ \line(1,0){15} \ O_2 \rightarrow~ \line(1,0){15} \ H_2O$

A. $2.02 \ g$

B. $20.2 \ g$

C. $10.1 \ g$

D. $90.0 \ g$

E. $180. \ g$

6. How many grams of calcium can be produced by the complete reaction of $9.35 \ grams$ of calcium oxide, according to following, as yet unbalanced, equation?

$\line(1,0){15} \ CaO~ +~ \line(1,0){15} \ C \rightarrow~ \line(1,0){15} \ Ca ~+~ \line(1,0){15} \ CO_2$

A. $6.70 \ g$

B. $3.34 \ g$

C. $12.4 \ g$

D. $7.19 \ g$

E. None of these.

7. In a particular reaction, iron (III) oxide and carbon solid reacted to produce iron metal and carbon monoxide. How many grams of iron (III) oxide are required to produce $150. \ grams$ of carbon monoxide?

A. $160. \ g$

B. $222 \ g$

C. $286 \ g$

D. $480. \ g$

E. None of these.

8. How many grams of octane, $C_8H_{18}$, when burned in oxygen gas are required to produce $272 \ grams$ of carbon dioxide? The other product is water.

A. $136 \ g$

B. $121 \ g$

C. $100. \ g$

D. $94.6 \ g$

E. $88.2 \ g$

9. How many grams of bromine gas would be liberated when $25.0 \ grams$ of gallium bromide were heated and decomposed to form gallium metal and bromine gas?

A. $16.4 \ g$

B. $19.4 \ g$

C. $21.8 \ g$

D. $27.1 \ g$

E. None of these.

10. $2000. \ g$ of potassium carbonate react completely with barium phosphate to produce potassium phosphate and barium carbonate. How many grams of barium carbonate will be formed?

A. $1240 \ g$

B. $1680 \ g$

C. $2220 \ g$

D. $2860 \ g$

E. None of these.

## Limiting Reactant Worksheet

CK-12 Foundation Chemistry

Name______________________ Date_________

1. If $2.5 \ moles$ of copper and $5.5 \ moles$ of silver nitrate are available to react in the following equation, what is the limiting reactant? (The equation is not yet balanced.)

$\line(1,0){15} \ Cu ~+~ \line(1,0){15} \ AgNO_3~ \rightarrow~ \line(1,0){15} \ ~Cu(NO_3)_2 ~+ ~\line(1,0){15} \ Ag$

A. copper

B. silver nitrate

C. copper (II) nitrate

D. silver

E. None of these.

2. How many grams of calcium hydroxide will be formed in the following reaction when $4.44 \ g$ of calcium oxide and $7.77 \ g$ of water are available to react? (The equation is not yet balanced.)

$\line(1,0){15} \ CaO ~+~ \line(1,0){15} \ H_2O \rightarrow \line(1,0){15} \ Ca(OH)_2$

A. $12.2 \ g$

B. $7.77 \ g$

C. $5.86 \ g$

D. $4.11 \ g$

E. None of these.

3. Magnesium undergoes a single replacement reaction with nitric acid, $HNO_3$. Write the balance equation for the reaction and determine how many grams of hydrogen gas will be formed from the reaction of $3.00 \ grams$ of magnesium with $18.00 \ grams$ of nitric acid.

A. $0.695 \ g$

B. $0.572 \ g$

C. $0.540 \ g$

D. $0.492 \ g$

E. None of these.

4. Sulfur reacts with oxygen gas to produce sulfur trioxide. Write the balanced equation for the reaction and determine how many grams of sulfur trioxide will be produced when $6.30 \ g$ of $S$ and $10.0 \ g$ of $O_2$ are available for reaction.

A. $16.3 \ g$

B. $15.7 \ g$

C. $13.2 \ g$

D. $11.9 \ g$

E. None of these.

5. Some of the acid in acid rain is produced from the following reaction:

$3 \ NO_2 + H_2O \rightarrow NO + 2 \ HNO_3$

A falling raindrop with a mass of $0.0500 \ gram$ comes into contact with $0.200 \ gram$ of $NO_2$. What mass of $HNO_3$ can be produced?

A. $0.183 \ g$

B. $0.250 \ g$

C. $0.350 \ g$

D. $0.146 \ g$

E. None of these.

6. In problem #5, how many grams of the excess reactant remains after the reaction?

A. $0.0415 \ g$

B. $0.0388 \ g$

C. $0.0264 \ g$

D. $0.0239 \ g$

E. None of these.

7. Consider the following reaction: $2 \ Al + 6 \ HBr \rightarrow 2 \ AlBr_3 + 3 \ H_2$. When $87.0 \ g$ of $Al$ is combined with $401 \ g$ of $HBr$, how many grams of $H_2$ are formed?

A. $3.89 \ g$

B. $5.01 \ g$

C. $7.11 \ g$

D. $12.4 \ g$

E. None of these.

## Percent Yield Worksheet

CK-12 Foundation Chemistry

Name______________________ Date_________

1. Methanol, $CH_3OH$ can be produced by the following reaction.

$2 \ H_2 + CO \rightarrow CH_3OH$

Assume $CO$ is the limiting reactant and $2.00 \ mols$ of $CO$ are used in the reaction. If $0.780 \ mols$ of $CH_3OH$ are produced by the reaction, what is the percent yield?

2. Consider the following reaction.

$3 \ Si + 2 \ N_2 \rightarrow Si_3N_4$

A. What is the theoretical yield of $Si_3N_4$ from this reaction when $21.45 \ mols$ of $Si$ are reacted with excess $N_2$?

B. If $5.92 \ mols$ of $Si_3N_4$ are actually produced, what is the percent yield?

3. Part of the $SO_2$ that is introduced into the atmosphere by the combustion of sulfur containing compounds ends up being converted to sulfuric acid, $H_2SO_4$ by the following reaction.

$2 \ SO_2 + O_2 + 2 \ H_2O \rightarrow 2 \ H_2SO_4$

A. What is the theoretical yield of $H_2SO_4$ if $100. \ g$ of $SO_2$ is completely consumed?

B. If the actual yield from the reaction in A is $100. \ g$ of $H_2SO_4$, what is the percent yield?

4. Consider the reaction: $4 \ FeS_2 + 11 \ O_2 \rightarrow 2 \ Fe_2 O_3 + 8 \ SO_2$

A. If $20.0 \ moles$ of $FeS_2$ react with $60.0 \ moles$ of $O_2$, what is the limiting reactant?

B. How many moles of $SO_2$ are formed?

C. How many moles of the reactant in excess will be left over at the end of the reaction?

D. If the actual yield of $SO_2$ is $25.0 \ moles$, what is the percent yield?

• The worksheet answer keys are available upon request. Please send an email to teachers-requests@ck12.org to request the worksheet answer keys.

Aug 18, 2012

Aug 13, 2014