4 HCI(g) + O₂(g) 2 Cl₂(g) + 2 H₂O(g) How many liters of HCI gas do I need to produce 37 liters of chlorine gas at STP? (Hint: Work this on paper first.) Answer= L 2 B5H₂(I) + 12 O₂(g) 5 B₂O3(s) + 9 H₂O(l) How many grams of B₂O3 can I produce if I react 72.5 liters of oxygen gas at STP? Answer= grams
4 HCI(g) + O₂(g) 2 Cl₂(g) + 2 H₂O(g) How many liters of HCI gas do I need to produce 37 liters of chlorine gas at STP? (Hint: Work this on paper first.) Answer= L 2 B5H₂(I) + 12 O₂(g) 5 B₂O3(s) + 9 H₂O(l) How many grams of B₂O3 can I produce if I react 72.5 liters of oxygen gas at STP? Answer= grams
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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![### Stoichiometry Problems
**Problem 1:**
\[ 4 \, \text{HCl}(g) + \text{O}_2(g) \rightarrow 2 \, \text{Cl}_2(g) + 2 \, \text{H}_2\text{O}(g) \]
**Question:**
How many liters of HCl gas do I need to produce 37 liters of chlorine gas at STP?
*(Hint: Work this on paper first.)*
**Answer:**
\[ \text{Answer} = \_\_\_\_\_\_ \, \text{L} \]
---
**Problem 2:**
\[ 2 \, \text{B}_5\text{H}_9(l) + 12 \, \text{O}_2(g) \rightarrow 5 \, \text{B}_2\text{O}_3(s) + 9 \, \text{H}_2\text{O}(l) \]
**Question:**
How many grams of \( \text{B}_2\text{O}_3 \) can I produce if I react 72.5 liters of oxygen gas at STP?
**Answer:**
\[ \text{Answer} = \_\_\_\_\_ \, \text{grams} \]
### Explanation
These problems are designed to test your ability to apply stoichiometry concepts. To solve them, you should:
1. Use the balanced chemical equations provided.
2. Calculate the molar ratios between reactants and products.
3. Apply the ideal gas law concepts, where required, assuming conditions are at Standard Temperature and Pressure (STP).
4. Convert between liters of gas and moles using the molar volume of a gas at STP (22.4 L/mol).
5. For problem 2, additionally convert moles of product to grams using its molar mass.
Work through these problems on paper using the steps above to determine the correct answers.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdada2ca3-6733-4968-8db7-4e672b70a8e4%2F98ab0fcc-f53e-468c-8476-46df157210cd%2Ftob2u88_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Stoichiometry Problems
**Problem 1:**
\[ 4 \, \text{HCl}(g) + \text{O}_2(g) \rightarrow 2 \, \text{Cl}_2(g) + 2 \, \text{H}_2\text{O}(g) \]
**Question:**
How many liters of HCl gas do I need to produce 37 liters of chlorine gas at STP?
*(Hint: Work this on paper first.)*
**Answer:**
\[ \text{Answer} = \_\_\_\_\_\_ \, \text{L} \]
---
**Problem 2:**
\[ 2 \, \text{B}_5\text{H}_9(l) + 12 \, \text{O}_2(g) \rightarrow 5 \, \text{B}_2\text{O}_3(s) + 9 \, \text{H}_2\text{O}(l) \]
**Question:**
How many grams of \( \text{B}_2\text{O}_3 \) can I produce if I react 72.5 liters of oxygen gas at STP?
**Answer:**
\[ \text{Answer} = \_\_\_\_\_ \, \text{grams} \]
### Explanation
These problems are designed to test your ability to apply stoichiometry concepts. To solve them, you should:
1. Use the balanced chemical equations provided.
2. Calculate the molar ratios between reactants and products.
3. Apply the ideal gas law concepts, where required, assuming conditions are at Standard Temperature and Pressure (STP).
4. Convert between liters of gas and moles using the molar volume of a gas at STP (22.4 L/mol).
5. For problem 2, additionally convert moles of product to grams using its molar mass.
Work through these problems on paper using the steps above to determine the correct answers.
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