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Consider the flasks in the following diagram. 2.00 L H2 1.00 L N2 425 torr 0.320 atm What are the final partial pressures of H2 and N2 after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L. PH, - torr PN2 torr What is the total pressure (in torr)? torr

Consider the flasks in the following diagram. 2.00 L H2 1.00 L N2 425 torr 0.320 atm What are the final partial pressures of H2 and N2 after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L. PH, - torr PN2 torr What is the total pressure (in torr)? torr

Chemistry
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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**Consider the flasks in the following diagram.** - Diagram description: The diagram shows two interconnected flasks. The left flask contains 2.00 L of H₂ at a pressure of 425 torr. The right flask contains 1.00 L of N₂ at a pressure of 0.320 atm. The two flasks are connected by a stopcock, which can be opened to allow the gases to mix. **What are the final partial pressures of H₂ and N₂ after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L.)** \[ P_{H₂} = \_\_\_\_ \text{torr} \] \[ P_{N₂} = \_\_\_\_ \text{torr} \] **What is the total pressure (in torr)?** \[ \_\_\_\_ \text{torr} \]
Transcribed Image Text:**Consider the flasks in the following diagram.** - Diagram description: The diagram shows two interconnected flasks. The left flask contains 2.00 L of H₂ at a pressure of 425 torr. The right flask contains 1.00 L of N₂ at a pressure of 0.320 atm. The two flasks are connected by a stopcock, which can be opened to allow the gases to mix. **What are the final partial pressures of H₂ and N₂ after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L.)** \[ P_{H₂} = \_\_\_\_ \text{torr} \] \[ P_{N₂} = \_\_\_\_ \text{torr} \] **What is the total pressure (in torr)?** \[ \_\_\_\_ \text{torr} \]
Expert Solution
Step 1

Given: Initial pressure of H2 = 425 torr

The initial volume of H2 = 2.00 L

The initial pressure of N2 = 0.320 atm = 0.320 × 760 = 243.2 torr                              (since 1 atm = 760 torr)

The initial volume of H2 = 1.00 L

And the final volume of gases = 3.00 L

 

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