Home
Class 11
CHEMISTRY
For a real gas (mol.mass =60) if density...

For a real gas (mol.mass =60) if density at critical point is `0.80g//cm^(-3)` and its `T_(c)=(4xx10^(5))/(821)K,` then van der Waals' constant a ( in atm `L^(2)mol^(-2)`) is

A

0.3375

B

3.375

C

1.68

D

0.025

Text Solution

Verified by Experts

The correct Answer is:
b
(b) `V_(c)=(60)/(0.80)=75cm^(3)mol^(-1),`
`b=(V_(c))/(3)=25cm^(3)mol^(-1)=0.025Lmol^(-1)`
`:." "T_(c)=(8a)/(27Rb)`
`(4xx10^(5))/(821)=(8xxa)/(27xx0.0821xx0.025)`
`implies" "a=3.375`
Promotional Banner

Topper's Solved these Questions

  • GASEOUS STATE

    NARENDRA AWASTHI|Exercise Level 1 (Q.31 To Q.60)|1 Videos

  • GASEOUS STATE

    NARENDRA AWASTHI|Exercise Level 1 (Q.121 To Q.150)|1 Videos

  • ELECTROCHEMISTRY

    NARENDRA AWASTHI|Exercise Level 3 - Subjective Problems|1 Videos

  • IONIC EEQUILIBRIUM

    NARENDRA AWASTHI|Exercise Assertin-Reason Type Questions|1 Videos

Similar Questions

Explore conceptually related problems

For a real gas 'X'the Boyle point is 240^@C . If the van der Waals constant 'b'is 0.08 dm^3 mol^(-1) , calculate the value of constant 'a'for 'X'.

The compression factor for one mole of real gas at 0^@C and 100 atm is 0.5. Calculate the van der Waals' constant 'a', if 'b' is zero.

2 moles of gas contained in a four litre flask exerts a pressure of Il atm at 27^@C . If vander Waals parameter bis 0.05 l/mol, the value of 'a' (in atm "lt"^(2) "mol"^(-2) ) is

The essential conditions for liquefaction of gases were discovered by Andrews in 1869 as a result of his study of pressure-volume-temperature relationship for CO_(2) . It was found that above a certain temperature, it was impossible to liquefy a gas whatever the pressure was applied. The temperature below which the gas can be liquefied by the application of pressure alone is called critical temperature (Tc). The pressure required to liquefy a gas at this temperature is called the critical pressure (Pc). The volume occupied by one mole of the substance at the critical temperature and pressure is called critical volume. Critical constants are related with van der waals' constant as follows: V_( c) = 3b, P_( c) =a/(27b^(2)), T_( c) =(8a)/(27 Rb) The values of critical volumes of four gases A, B, C and D are 0.025L, 0.312L, 0.245L and 0.432L respectively. The gas with larger molecular diameter will be :

The table indicates the value of vander Waal's constant a in L^(2) atm mol 2. The gas which can most easily be liquefied is ?

The rate constants for a reaction at 400 K and 500 K are 2 . 60 xx 10^(-5) s^(-1) and 2.60 xx 10^(-3) s^(-1) respectively. The activation energy of the reaction in kJ mol^(-1) is

The rate constant of a reaction is 2.5xx10^(-2)" L mol"^(-1)s^(-1) . Calculate the initial rate with concentration 0.2" mol L"^(-1) .