Home
Class 12
CHEMISTRY
The unit of van der Waals constant 'a' i...

The unit of van der Waals constant 'a' is

A

atm` * L * mol^(-2)`

B

atm `* L^(2) * mol^(-2)`

C

atm `* L^(2) * mol^(-1)`

D

atm`* L`

Text Solution

Verified by Experts

Promotional Banner

Topper's Solved these Questions

  • MODEL QUESTIONS PAPER

    CHHAYA PUBLICATION|Exercise SET II ( SECTION II ) ( GROUP A)|6 Videos

  • MODEL QUESTIONS PAPER

    CHHAYA PUBLICATION|Exercise SET II ( SECTION II ) ( GROUP B)|7 Videos

  • MODEL QUESTIONS PAPER

    CHHAYA PUBLICATION|Exercise SET I (SECTION II ) (GROUP D)|11 Videos

  • MODEL QUESTION PAPER

    CHHAYA PUBLICATION|Exercise Answer the following question (set-3)|130 Videos

  • ORGANIC CHEMISTRY : BASIC PRINCIPLES AND TECHNIQUES

    CHHAYA PUBLICATION|Exercise WARM UP EXERICSE|132 Videos

Similar Questions

Explore conceptually related problems

Write the units of van der waals constants 'a' and 'b'.

Write the units of van der waals constants 'a' and 'b',- what are the significances of 'a' and 'b' ?

(i) Explain the nature of the graphs of logP versus log V and logV versus logT. (ii) What are the units of the van der waals constant 'a' and 'b' ?

(a) State Dalton's law of partial pressure. (b) The value of van der waals constant 'a' for N_(2) and NH_(3) are 1.37 and 4.30L^(2)*atm*mol^(-2) respectively. Explain the difference in values.

The values of van der waals constants 'a' and 'b' for X, Y, and Z gases are 6,6,20 and 0.025, 0.15, 0.11, respectively. Which one has the highest critical temperature ?

Write the units of Vander Waals constants a and b.

The vlaue of van der waals constant 'a' for nitrogen gas is 1.37L^(2)*atm*mol^(-2) , but that for ammonia gas is 4.30L^(2)*atm*mol^(-2) . What is the reason for this large difference ? Which one of these two gases would you expect to have higher critical temperature?

The critical temperature of NH_(3) and SO_(2) gases are 405.0 K and 430.3K, respectively. For which gas is the value of van der waals constant 'a' greater. And why?

(i) Any real gas behaves ideally at very low pressure and high temperature explain. (ii) The value of van der waals constant 'a' for N_(2) and NH_(3) are 1.37 and 4.30 L^(2)*atm*mol^(-2) respectively explain the difference in values.

Compressibility factor of 2 mol of NH_(3) gas at 27^(@)C and 9.18 atm pressure is 0.931. if the volume of the gas molecules is not taken into consideration, then what is the value of van der waals constant 'a' for NH_(3) gas?