CHEMISTRY
2nd Edition
ISBN: 9781593995782
Author: OpenStax
Publisher: XANEDU PUBLISHING
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Textbook Question
Chapter 9, Problem 70E
Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas.
(a) Outline the steps necessary to answer the following question: What volume of
(b) Answer the question.
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3. Hydrochloric acid is a strong acid that can be used to make sodium chloride and a weak acid, nitrous acid. Write the
balanced chemical equation of this reaction. (You can use the information in part b to help you determine states),
b. Using the information below determine the AºHrn of the gencration of nitrous acid and sodium chloride.
2NACI (s) + H;O (1) → 2HCI (aq) + Na;O (aq)
AH, = 507.1 kJ/mol
NO (g) + NO2 (g) → Na;O (aq) + 2NaNO; (aq)
AH,n = -427.4 kJ/mol
NO (g) + NO2 (g) →N20 (g) +
AHrxn = -42.8 kJ/mol
(8)
2HNO2 (aq)
→ N20 (g) + O2 (g) + H2O (I)
AHrn = 34.2 kJ/mol
The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large
volumes of nitrogen gas.
1. Write a balanced chemical equation, including physical state symbols, for the
decomposition of solid sodium azide (NaN,) into solid sodium and gaseous dinitrogen.
alb
Ar
2. Suppose 12.0 L of dinitrogen gas are produced by this reaction, at a temperature of
13.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must
have reacted. Round your answer to 3 significant digits.
Explanation
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A 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at 23 oC and an atmospheric pressure of 756 mm Hg. The hydrogen gas is collected over water.
Write a balanced chemical equation for the reaction between solid aluminum metal and aqueous hydrochloric acid.
Using stoichiometry, determine the theoretical yield of hydrogen gas (in moles) that will be produced by the complete reaction of the aluminum metal.
Refer to Table 1 and calculate the partial pressure of hydrogen gas.
Temperature
Pressure
Temperature
Pressure
Temperature
Pressure
16 °C
14 mm Hg
21 °C
19 mm Hg
26 °C
24 mm Hg
17 °C
15 mm Hg
22 °C
20 mm Hg
27 °C
25 mm Hg
18 °C
16 mm Hg
23 °C
21 mm Hg
28 °C
26 mm Hg
19 °C
17 mm Hg
24 °C
22 mm Hg
29 °C
27 mm Hg
20 °C
18 mm Hg
25 °C
23 mm Hg
30 °C
28 mm Hg
Using the Ideal Gas Law, determine the experimental moles of hydrogen gas…
Chapter 9 Solutions
CHEMISTRY
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