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14.5: Multimedia Resources for Chapter 14

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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?

Answers to Worksheets

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

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Aug 18, 2012

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Jul 21, 2014
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