Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed. 2NAN, (s) → 2Na(s) + 3N,(g) What mass of sodium azide is required to produce 2.6 ft (73.6 L) of nitrogen gas with a density of 1.25 g/L?
Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed. 2NAN, (s) → 2Na(s) + 3N,(g) What mass of sodium azide is required to produce 2.6 ft (73.6 L) of nitrogen gas with a density of 1.25 g/L?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Educational Content on Stoichiometry and Yield Calculations**
1. **Chemical Reaction Calculation**
- Calculate the amount of product formed from reactants. Use stoichiometry to balance equations and convert units when necessary.
2. **Reaction of CuCl₂ and KI**
- Balanced equation: \(2 \text{CuCl}_2 + 4 \text{KI} \rightarrow 2 \text{CuI} + 4 \text{KCl} + I_2\)
- Determine the mass of \(I_2\) produced from 0.4235 mol of CuCl₂.
- (a) Calculate number of molecules of \(I_2\) produced.
- (b) Calculate the mass of \(I_2\) produced.
3. **Formation of Silver Oxide**
- What mass of silver oxide, Ag₂O, is required to produce 250 g of silver sulfadiazine, AgC₁₀H₉N₄SO₂?
- Balanced equation: 2 Ag₂O + AgC₁₀H₉N₄SO₂ + H₂O
4. **Inflation of Automotive Air Bags**
- Sodium azide, NaN₃, is decomposed to produce \(N_2\) gas.
- Equation: \(2 \text{NaN}_3 (s) \rightarrow 2 \text{Na} (s) + 3 \text{N}_2 (g)\)
- Calculate the mass of \(NaN₃\) required to produce nitrogen with a density of 1.25 g/L.
5. **Percent Yield Calculation**
- Given: 53.6 g of CO₂ obtained from heating 1.31 g of CaCO₃.
- Calculate percent yield:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100
\]
- Example calculated yield: 92.4%
6. **Laboratory Experiment**
- Reaction: \(3.0 \text{ mol HF} \) produced from 0.10 mol HI.
- Calculate the percent yield.
7. **Limiting Reactant and Theoretical Yield**
- 3.00 g of propane, \(C_](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe33c485d-9ded-4ed9-b52c-b6396698c059%2Ff63693c5-6c5d-4029-974c-213439ce223a%2Fn1jxme7.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content on Stoichiometry and Yield Calculations**
1. **Chemical Reaction Calculation**
- Calculate the amount of product formed from reactants. Use stoichiometry to balance equations and convert units when necessary.
2. **Reaction of CuCl₂ and KI**
- Balanced equation: \(2 \text{CuCl}_2 + 4 \text{KI} \rightarrow 2 \text{CuI} + 4 \text{KCl} + I_2\)
- Determine the mass of \(I_2\) produced from 0.4235 mol of CuCl₂.
- (a) Calculate number of molecules of \(I_2\) produced.
- (b) Calculate the mass of \(I_2\) produced.
3. **Formation of Silver Oxide**
- What mass of silver oxide, Ag₂O, is required to produce 250 g of silver sulfadiazine, AgC₁₀H₉N₄SO₂?
- Balanced equation: 2 Ag₂O + AgC₁₀H₉N₄SO₂ + H₂O
4. **Inflation of Automotive Air Bags**
- Sodium azide, NaN₃, is decomposed to produce \(N_2\) gas.
- Equation: \(2 \text{NaN}_3 (s) \rightarrow 2 \text{Na} (s) + 3 \text{N}_2 (g)\)
- Calculate the mass of \(NaN₃\) required to produce nitrogen with a density of 1.25 g/L.
5. **Percent Yield Calculation**
- Given: 53.6 g of CO₂ obtained from heating 1.31 g of CaCO₃.
- Calculate percent yield:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100
\]
- Example calculated yield: 92.4%
6. **Laboratory Experiment**
- Reaction: \(3.0 \text{ mol HF} \) produced from 0.10 mol HI.
- Calculate the percent yield.
7. **Limiting Reactant and Theoretical Yield**
- 3.00 g of propane, \(C_
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