Problem: Explain the negative deviation from ideal gas behavior of N2 below 300 atm in the figure on the left. 

🤓 Based on our data, we think this question is relevant for Professor Atwood's class at UB.

FREE Expert Solution

In this problem, we are asked to explain the negative deviation from the ideal gas behavior of N2 below 300 atm.

The deviation from the ideal gas behavior is expressed introducing a factor in the ideal gas equation. 

This is the compressibility factor (Z) which is expressed as:

Z=PVnRT

Where:
          For ideal gas:  Z = 1 
          For real gas: Z 1 


In the case of real gases:

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Problem Details

Explain the negative deviation from ideal gas behavior of N2 below 300 atm in the figure on the left. 

A graph showing that nitrogen behaves more like an ideal gas at higher temperatures. It has pressure in atmospheres on the x-axis, ranging from 0 to 900 with intervals of 300. PV divided by RT is on the y-axis, ranging from 0 to 3 with intervals of 1. Curves are plotted for an ideal gas, which is a dashed horizontal line at 1.0 PV divided by RT, and for nitrogen at 200 Kelvin, 500 Kelvin, and 1000 Kelvin. The curve for 1000 Kelvin most approximates the ideal, while the curve for 200 Kelvin diverges most.

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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 Kinetic Molecular Theory concept. You can view video lessons to learn Kinetic Molecular Theory. Or if you need more Kinetic Molecular Theory practice, you can also practice Kinetic Molecular Theory practice problems.

What professor is this problem relevant for?

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