3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H₂O In the above equation how many moles of water can be made when 173.9 grams of HNO3 are consumed? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Molar Element Mass Hydrogen 1 Nitrogen 14 Copper 63.5 Oxygen 16
3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H₂O In the above equation how many moles of water can be made when 173.9 grams of HNO3 are consumed? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Molar Element Mass Hydrogen 1 Nitrogen 14 Copper 63.5 Oxygen 16
Chemistry
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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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![### Problem Statement:
In the above equation, how many moles of water can be made when 173.9 grams of HNO₃ are consumed?
Round your answer to the nearest tenth. If your answer is a whole number like 4, report the answer as 4.0.
#### Chemical Equation:
\[ 3 \text{Cu} + 8 \text{HNO}_3 \rightarrow 3 \text{Cu(NO}_3\text{)}_2 + 2 \text{NO} + 4 \text{H}_2\text{O} \]
#### Given Information:
Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.:
- **Element**: **Molar Mass**
- Hydrogen \( \text{H} \): 1
- Nitrogen \( \text{N} \): 14
- Copper \( \text{Cu} \): 63.5
- Oxygen \( \text{O} \): 16
### Calculation Steps:
1. **Determine the molar mass of HNO₃**:
- Hydrogen (H): \( 1 \times 1 = 1 \)
- Nitrogen (N): \( 1 \times 14 = 14 \)
- Oxygen (O): \( 3 \times 16 = 48 \)
- Total molar mass of HNO₃: \( 1 + 14 + 48 = 63 \text{ g/mol} \)
2. **Calculate the number of moles of HNO₃**:
\[
\text{Moles of HNO}_3 = \frac{\text{Mass of HNO}_3}{\text{Molar Mass of HNO}_3} = \frac{173.9 \text{ grams}}{63 \text{ g/mol}} = 2.76 \text{ moles}
\]
3. **Use stoichiometry to determine moles of water produced**:
- According to the balanced equation \( 8 \text{ moles of HNO}_3 \) produces \( 4 \text{ moles of H}_2\text{O} \).
- Therefore, \( 2.76 \text{ moles of HNO}_3 \) will produce:
\[](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe365b4d4-2c32-4fdf-8435-ed630ab2ec26%2F15b29ac0-a252-4adf-bbcc-1958429f1793%2Fkdd35gp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Problem Statement:
In the above equation, how many moles of water can be made when 173.9 grams of HNO₃ are consumed?
Round your answer to the nearest tenth. If your answer is a whole number like 4, report the answer as 4.0.
#### Chemical Equation:
\[ 3 \text{Cu} + 8 \text{HNO}_3 \rightarrow 3 \text{Cu(NO}_3\text{)}_2 + 2 \text{NO} + 4 \text{H}_2\text{O} \]
#### Given Information:
Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.:
- **Element**: **Molar Mass**
- Hydrogen \( \text{H} \): 1
- Nitrogen \( \text{N} \): 14
- Copper \( \text{Cu} \): 63.5
- Oxygen \( \text{O} \): 16
### Calculation Steps:
1. **Determine the molar mass of HNO₃**:
- Hydrogen (H): \( 1 \times 1 = 1 \)
- Nitrogen (N): \( 1 \times 14 = 14 \)
- Oxygen (O): \( 3 \times 16 = 48 \)
- Total molar mass of HNO₃: \( 1 + 14 + 48 = 63 \text{ g/mol} \)
2. **Calculate the number of moles of HNO₃**:
\[
\text{Moles of HNO}_3 = \frac{\text{Mass of HNO}_3}{\text{Molar Mass of HNO}_3} = \frac{173.9 \text{ grams}}{63 \text{ g/mol}} = 2.76 \text{ moles}
\]
3. **Use stoichiometry to determine moles of water produced**:
- According to the balanced equation \( 8 \text{ moles of HNO}_3 \) produces \( 4 \text{ moles of H}_2\text{O} \).
- Therefore, \( 2.76 \text{ moles of HNO}_3 \) will produce:
\[
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