How many grams of phosphoric acid (97.99 g/mol) can be produced from the reaction of 10.0 g o P4010 (283.9 g/mol) with 5.00 grams of water (18.02 g/mol) according to the following balanced reaction? P4010(s) + 6 H₂O(l) → 4 H3PO4(aq) 15.0 g 18.1 g 13.8 g
How many grams of phosphoric acid (97.99 g/mol) can be produced from the reaction of 10.0 g o P4010 (283.9 g/mol) with 5.00 grams of water (18.02 g/mol) according to the following balanced reaction? P4010(s) + 6 H₂O(l) → 4 H3PO4(aq) 15.0 g 18.1 g 13.8 g
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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![### Chemical Reaction Problem
**Question:**
How many grams of phosphoric acid (97.99 g/mol) can be produced from the reaction of 10.0 g of P\(_4\)O\(_{10}\) (283.9 g/mol) with 5.00 grams of water (18.02 g/mol) according to the following balanced reaction?
\[ \text{P}_4\text{O}_{10(s)} + 6 \text{H}_2\text{O}_{(l)} \rightarrow 4 \text{H}_3\text{PO}_{4(aq)} \]
**Options:**
- 15.0 g
- 18.1 g
- 13.8 g
### Explanation:
To solve this, follow these steps:
1. **Calculate the moles of P\(_4\)O\(_{10}\) and H\(_2\)O**:
- Moles of P\(_4\)O\(_{10}\) = \(\frac{10.0 \ \text{g}}{283.9 \ \text{g/mol}}\)
- Moles of H\(_2\)O = \(\frac{5.00 \ \text{g}}{18.02 \ \text{g/mol}}\)
2. **Determine the limiting reagent**:
- The balanced chemical equation shows that 1 mole of P\(_4\)O\(_{10}\) reacts with 6 moles of H\(_2\)O to produce 4 moles of H\(_3\)PO\(_4\).
3. **Use the stoichiometry of the reaction to find the moles of H\(_3\)PO\(_4\)**:
- Using the moles of the limiting reagent, calculate the moles of H\(_3\)PO\(_4\) produced.
4. **Convert moles of H\(_3\)PO\(_4\) to grams**:
- Grams of H\(_3\)PO\(_4\) = moles of H\(_3\)PO\(_4\) \(\times\) molar mass of H\(_3\)PO\(_4\) (97.99 g/mol).
By working through these steps, you can determine](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9de95467-8766-4670-8442-783f9816c074%2F54f678ad-d210-4a41-8c4f-d6773a54c4e4%2Ftw4m1il_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction Problem
**Question:**
How many grams of phosphoric acid (97.99 g/mol) can be produced from the reaction of 10.0 g of P\(_4\)O\(_{10}\) (283.9 g/mol) with 5.00 grams of water (18.02 g/mol) according to the following balanced reaction?
\[ \text{P}_4\text{O}_{10(s)} + 6 \text{H}_2\text{O}_{(l)} \rightarrow 4 \text{H}_3\text{PO}_{4(aq)} \]
**Options:**
- 15.0 g
- 18.1 g
- 13.8 g
### Explanation:
To solve this, follow these steps:
1. **Calculate the moles of P\(_4\)O\(_{10}\) and H\(_2\)O**:
- Moles of P\(_4\)O\(_{10}\) = \(\frac{10.0 \ \text{g}}{283.9 \ \text{g/mol}}\)
- Moles of H\(_2\)O = \(\frac{5.00 \ \text{g}}{18.02 \ \text{g/mol}}\)
2. **Determine the limiting reagent**:
- The balanced chemical equation shows that 1 mole of P\(_4\)O\(_{10}\) reacts with 6 moles of H\(_2\)O to produce 4 moles of H\(_3\)PO\(_4\).
3. **Use the stoichiometry of the reaction to find the moles of H\(_3\)PO\(_4\)**:
- Using the moles of the limiting reagent, calculate the moles of H\(_3\)PO\(_4\) produced.
4. **Convert moles of H\(_3\)PO\(_4\) to grams**:
- Grams of H\(_3\)PO\(_4\) = moles of H\(_3\)PO\(_4\) \(\times\) molar mass of H\(_3\)PO\(_4\) (97.99 g/mol).
By working through these steps, you can determine
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