Problem: Dry nitrogen gas is bubbled through liquid benzene (C 6H6) at 20.0 ˚C. From 100.0 L of the gaseous mixture of nitrogen and benzene, 24.7 g benzene is condensed by passing the mixture through a trap at a temperature where nitrogen is gaseous and the vapor pressure of benzene is negligible. What is the vapor pressure of benzene at 20.0 ˚C?

FREE Expert Solution

To calculate the vapor pressure of benzene (C6H6), we’re going to use the ideal gas equation:


Given:

Mass C6H6 = 24.7 g
Temperature = 20.0°C +273.15 K = 293.15 K
V = 100.0 L


Calculate moles C6H6:

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Problem Details

Dry nitrogen gas is bubbled through liquid benzene (C 6H6) at 20.0 ˚C. From 100.0 L of the gaseous mixture of nitrogen and benzene, 24.7 g benzene is condensed by passing the mixture through a trap at a temperature where nitrogen is gaseous and the vapor pressure of benzene is negligible. What is the vapor pressure of benzene at 20.0 ˚C?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

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Based on our data, we think this problem is relevant for Professor Cruz's class at USF.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.