1. Chemical Quantities and Aqueous Reactions
Clicker Questions
Chapter 4
Chemical Quantities and Aqueous Reactions
Allison Soult
University of Kentucky

2. How many moles of CO2 are produced when 3 moles of pentane react with excess oxygen? C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(l)
5 moles
3/5 moles
15 moles
3 moles
Answer: c

3. The overall equation involved in photosynthesis is
The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2. How many grams of glucose (C6H12O6, g/mol) form when 4.40 g of CO2 react?
18.0 g
3.00 g
108 g g
Answer: b

4. The rapid decomposition of sodium azide, NaN3, to its elements is one of the reactions used to inflate airbags: 2 NaN3 (s)  2 Na (s) + 3 N2 (g) How many grams of N2 are produced from 6.00 g of NaN3?
3.88 g
1.72 g
0.138 g
2.59 g
Answer: a

5. The overall equation involved in photosynthesis is
The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2. How many grams of carbon dioxide (CO2) are required to produce 18.0 g of C6H12O6?
18.0 g
3.00 g
54.0 g
26.4 g
4.40 g
Answer: d

6. Ammonia is produced using the Haber process:
Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 Calculate the mass of ammonia produced when 35.0 g of nitrogen react with 12.5 g of hydrogen.
47.5 g
42.6 g
35.0 g
63.8 g
70.5 g
Answer: b

7. Ammonia is produced using the Haber process:
Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 What percent yield of ammonia is produced from 15.0 kg each of H2 and N2, if 13.7 kg of product are recovered? Assume the reaction goes to completion.
7.53 × 10–2 %
1.50 × 10–1 %
75.3%
15.0%
16.2%
Answer: c

8. What mass of TiCl4 is needed to produce 25
What mass of TiCl4 is needed to produce 25.0 g of Ti if the reaction proceeds with an 82% yield? TiCl4 + 2Mg  Ti + 2 MgCl2
30.5 g
121 g
99.1 g
81.2 g
Answer: b

9. What is the molarity of an aqueous solution containing 22
What is the molarity of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution? M
1.85 × 10–3 M
1.85 M
3.52 M
0.104 M
Answer: c

10. Sulfuric acid is found in some types of batteries. What volume of 3
Sulfuric acid is found in some types of batteries. What volume of 3.50 M H2SO4 is required to prepare mL of 1.25 M H2SO4?
17.5 mL
700. mL
89.3 mL
109 mL
None of the above
Answer: c

11. A 45.0 mL solution is M HCl. What is the concentration after 25.0 mL of water is added to the solution? Assume volumes are additive.
0.321 M
0.179 M
0.900 M
0.278 M
Answer: a

12. Which of the following aqueous solutions would conduct electricity?
AgNO3
C11H22O11 (sucrose)
CH3CH2OH (ethanol)
All of the above
None of the above
Answer: a

13. Which of the following compounds will be insoluble in water?
Ca(OH)2
Na3PO4
CaS
Hg2Cl2
LiF
Answer: d

14. What is the maximum number of grams of PbI2 precipitated upon mixing 25.0 mL of M KI with 15.0 mL of M Pb(NO3)2?
0.864 g
1.73 g
1.21 g
2.07 g
None of the above
Answer: a

15. What is the product, if any, when AgNO3 and NaCl react in aqueous solution?
AgCl
NaNO3
No precipitate
Answer: c

16. A 25. 0 mL sample of H2SO4 is neutralized with NaOH
A 25.0 mL sample of H2SO4 is neutralized with NaOH. What is the concentration of the H2SO4 if 35.0 mL of M NaOH are required to completely neutralize the acid?
0.210 M
0.105 M
0.150 M
0.420 M
None of the above
Answer: b

17. What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize L of M H2SO4?
2.94 × 104 g
1.47 × 104 g
5.88 × 104 g
3.50 × 103 g
1.75 × 103 g
Answer: c

18. Determine the oxidation number of the red element in each of the following compounds: H2PO4– SO32– N2O4
Answer: c

19. Which of the following is a redox reaction?
HBr (aq) + KOH (aq) → H2O (l) + KBr (aq)
SO3 (g) + H2O (l) → H2SO4 (aq)
HBr (aq) + Na2S (aq) → NaBr (aq) + H2S (g)
NH4+ (aq) + 2 O2 (g) → H2O (l) + NO3– (aq) + 2 H+ (aq)
None of the above
Answer: d

20. What is the reducing agent in the following reaction
What is the reducing agent in the following reaction? Zn + 2 MnO2 + 2 H2O → Zn(OH)2 + 2 MnO(OH) Zn
MnO2
H2O
Zn(OH)2
MnO(OH)
Answer: a