In questions 5 and 6, assume 1.00 mol of any gas occupies 22.40 L at standard temperature and pressure (STP). 5. What volume of hydrogen gas is obtained when 9.62 g of chromium metal reacts with an excess of dilute sulfuric acid at STP? 2 Crs) + 3 H2 SO4 (aq) Cr2 (SO4)3 (aq) + 3 H2 (g) 6. What volume of oxygen, at STP, is required to burn exactly 1.58 L of methane (CH4 (9), according to the reaction below? CH4 (g) + 202 (g) CO2 (9) + 2H2O (9)
In questions 5 and 6, assume 1.00 mol of any gas occupies 22.40 L at standard temperature and pressure (STP). 5. What volume of hydrogen gas is obtained when 9.62 g of chromium metal reacts with an excess of dilute sulfuric acid at STP? 2 Crs) + 3 H2 SO4 (aq) Cr2 (SO4)3 (aq) + 3 H2 (g) 6. What volume of oxygen, at STP, is required to burn exactly 1.58 L of methane (CH4 (9), according to the reaction below? CH4 (g) + 202 (g) CO2 (9) + 2H2O (9)
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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5 & 6 go together.
![**Educational Content on Gas Reactions and Calculations at STP**
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In questions 5 and 6, assume 1.00 mol of any gas occupies 22.40 L at standard temperature and pressure (STP).
**5. Hydrogen Gas Production Reaction**
- **Problem Statement**: What volume of hydrogen gas is obtained when 9.62 g of chromium metal reacts with an excess of dilute sulfuric acid at STP?
- **Chemical Reaction**:
\[
2 \text{Cr}_{(s)} + 3 \text{H}_2\text{SO}_4{}_{(aq)} \rightarrow \text{Cr}_2(\text{SO}_4)_3{}_{(aq)} + 3 \text{H}_2{}_{(g)}
\]
**6. Oxygen Volume for Methane Combustion**
- **Problem Statement**: What volume of oxygen, at STP, is required to burn exactly 1.58 L of methane (\(\text{CH}_4{}_{(g)}\)), according to the reaction below?
- **Chemical Reaction**:
\[
\text{CH}_4{}_{(g)} + 2\text{O}_2{}_{(g)} \rightarrow \text{CO}_2{}_{(g)} + 2\text{H}_2\text{O}_{(g)}
\]
**7. Gas Diffusion Comparison**
- **Problem Statement**: How much faster does \(\text{N}_2\) gas escape through a porous container than \(\text{Kr}\)?
**8. Pressure Calculation in a Tube**
- **Problem Statement**: Calculate the pressure inside a tube, given that the tube’s volume is 4.0 L, its temperature is 22 °C, and it contains 1.57 mg of hydrogen gas.
---
This content covers gas reactions involving chromium and sulfuric acid as well as methane combustion, providing a comprehensive overview of calculating gas volumes and pressures at standard conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7de42a67-181a-4f2f-af21-0f59713bb114%2F9f0fc1ed-09d3-47cd-b28b-cf126229c61b%2F0r4hgqj.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content on Gas Reactions and Calculations at STP**
---
In questions 5 and 6, assume 1.00 mol of any gas occupies 22.40 L at standard temperature and pressure (STP).
**5. Hydrogen Gas Production Reaction**
- **Problem Statement**: What volume of hydrogen gas is obtained when 9.62 g of chromium metal reacts with an excess of dilute sulfuric acid at STP?
- **Chemical Reaction**:
\[
2 \text{Cr}_{(s)} + 3 \text{H}_2\text{SO}_4{}_{(aq)} \rightarrow \text{Cr}_2(\text{SO}_4)_3{}_{(aq)} + 3 \text{H}_2{}_{(g)}
\]
**6. Oxygen Volume for Methane Combustion**
- **Problem Statement**: What volume of oxygen, at STP, is required to burn exactly 1.58 L of methane (\(\text{CH}_4{}_{(g)}\)), according to the reaction below?
- **Chemical Reaction**:
\[
\text{CH}_4{}_{(g)} + 2\text{O}_2{}_{(g)} \rightarrow \text{CO}_2{}_{(g)} + 2\text{H}_2\text{O}_{(g)}
\]
**7. Gas Diffusion Comparison**
- **Problem Statement**: How much faster does \(\text{N}_2\) gas escape through a porous container than \(\text{Kr}\)?
**8. Pressure Calculation in a Tube**
- **Problem Statement**: Calculate the pressure inside a tube, given that the tube’s volume is 4.0 L, its temperature is 22 °C, and it contains 1.57 mg of hydrogen gas.
---
This content covers gas reactions involving chromium and sulfuric acid as well as methane combustion, providing a comprehensive overview of calculating gas volumes and pressures at standard conditions.
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