🤓 Based on our data, we think this question is relevant for Professor Brunold's class at UW-MADISON.

Solution: Consider the flasks in the following diagram. What are the final partial pressures of H 2 and N2 after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L.) What is the total pressure (in torr)?

Problem

Consider the flasks in the following diagram. What are the final partial pressures of H 2 and N2 after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L.) What is the total pressure (in torr)?

Solution

Recall: The ideal gas law is as follows:

We can see that the pressure and volume of a gas are related to the number of moles of gas, the universal gas constant, and the temperature of the gas.

For a given number of moles of gas at a constant temperature, the initial and final pressure and volume of the gas are related by Boyle's law.

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