One litre of a gas at 300 atm and 473 K is compressed to a pressure of 600 atm and 273 K. The

Name: Problem 37, Chapter 1: Numerical problems in Physical Chemistry for IIT-JEE
Uploaded: 2021-08-27T12:10:19-08:00
Duration: 1 min 50 s
Channel: Vishnu P
Description: One litre of a gas at 300 atm and 473 K is compressed to a pressure of 600 atm and 273 K. The compressibility factors found to be 1.072 and 1.375 respectively at the initial and finally conditions. Calculate the final volume.

step 1 Hi old again welcome to numerate and here we have a question to apply the equation compressibili

Question

One litre of a gas at 300 atm and $473 \mathrm{~K}$ is compressed to a pressure of 600 atm and $273 \mathrm{~K}$. The compressibility factors found to be $1.072$ and $1.375$ respectively at the initial and finally conditions. Calculate the final volume.

   One litre of a gas at 300 atm and $473 \mathrm{~K}$ is compressed to a pressure of 600 atm and $273 \mathrm{~K}$. The compressibility factors found to be $1.072$ and $1.375$ respectively at the initial and finally conditions. Calculate the final volume.

Numerical problems in Physical Chemistry for IIT-JEE

P. Bahadur, Shalabh… 2010 Edition

Chapter 1, Problem 37

Instant Answer

Solved by Expert Vishnu P

08/27/2021

Step 1

We can write this equation for the initial and final conditions as follows: $Z_1=\frac{P_1V_1}{RT_1}$ and $Z_2=\frac{P_2V_2}{RT_2}$. Show more…

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One litre of a gas at 300 atm and $473 \mathrm{~K}$ is compressed to a pressure of 600 atm and $273 \mathrm{~K}$. The compressibility factors found to be $1.072$ and $1.375$ respectively at the initial and finally conditions. Calculate the final volume.

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Key Concepts

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates a gas's pressure, volume, temperature, and number of moles. It assumes that gas molecules do not interact and occupy negligible space, providing a basic model for understanding gas behavior under many conditions.

Compressibility Factor

The compressibility factor (Z) is a correction factor that quantifies how much a real gas deviates from ideal behavior. It is defined by the equation Z = (PV)/(nRT) and is used to adjust ideal gas calculations to account for interactions between molecules and finite molecular volumes in real gases.

Real Gas Behavior

Real gas behavior acknowledges that gases do not always follow the ideal gas law, especially under high pressures or low temperatures where molecular interactions and volumes become significant. Adjusting calculations using factors like Z leads to improved accuracy in predicting the state properties of actual gases.

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