If 15.2 g N2 and 1.65 g H2 react to produce 1.33 g NH3, what is the percent yield of the reaction? N2(g) + 3 H2(g)→2 NH3(g) O 0.143 % O 7.20 % O 697 % O 14.4 % 14.3 %
If 15.2 g N2 and 1.65 g H2 react to produce 1.33 g NH3, what is the percent yield of the reaction? N2(g) + 3 H2(g)→2 NH3(g) O 0.143 % O 7.20 % O 697 % O 14.4 % 14.3 %
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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![**Chemistry: Calculating Percent Yield**
**Problem Statement:**
If \( 15.2 \, \text{g} \, \text{N}_2 \) and \( 1.65 \, \text{g} \, \text{H}_2 \) react to produce \( 1.33 \, \text{g} \, \text{NH}_3 \), what is the percent yield of the reaction?
\[ \text{N}_2(g) + 3 \, \text{H}_2(g) \rightarrow 2 \, \text{NH}_3(g) \]
**Options:**
- \( 0.143\% \)
- \( 7.20\% \)
- \( 697\% \)
- \( 14.4\% \)
- \( 14.3\% \)
**Instructions:**
Calculate the percent yield using the given masses and the chemical equation. Remember, percent yield is calculated using the formula:
\[
\text{Percent Yield} = \left(\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\right) \times 100\%
\]
Determine the theoretical yield based on stoichiometry and compare it with the actual yield provided.
---
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Transcribed Image Text:**Chemistry: Calculating Percent Yield**
**Problem Statement:**
If \( 15.2 \, \text{g} \, \text{N}_2 \) and \( 1.65 \, \text{g} \, \text{H}_2 \) react to produce \( 1.33 \, \text{g} \, \text{NH}_3 \), what is the percent yield of the reaction?
\[ \text{N}_2(g) + 3 \, \text{H}_2(g) \rightarrow 2 \, \text{NH}_3(g) \]
**Options:**
- \( 0.143\% \)
- \( 7.20\% \)
- \( 697\% \)
- \( 14.4\% \)
- \( 14.3\% \)
**Instructions:**
Calculate the percent yield using the given masses and the chemical equation. Remember, percent yield is calculated using the formula:
\[
\text{Percent Yield} = \left(\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\right) \times 100\%
\]
Determine the theoretical yield based on stoichiometry and compare it with the actual yield provided.
---
**Interface Elements:**
- **Submit Answer:** Button to confirm and submit your selected option.
- **Try Another Version:** Button to attempt a different variation of the problem.
- **Attempts Remaining:** Indicator showing that there are 3 attempts remaining for this item.
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