wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Calculate the pressure exerted by one mole of CO2 gas at 273 K if the van der Waal's constant, a=3.592 dm6 atm mol−2. Assume that the volume occupied by CO2 molecules is negligible.

A
0.9922 atm
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
1.9922 atm
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
9.9222 atm
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
0.1922 atm
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A 0.9922 atm

Van der Waals' equation for one mole of a gas is
[P+aV2](Vb)=RT.....(1)
Given that volume occupied by CO2 molecules, 'b' = 0 Hence, (1) becomes [P+aV2]V=RT or P=RTVaV2
Using R = 0.082, T = 273K, V =22.4 L for one mole of an ideal gas at 1 atm pressure.
P=0.082×27322.43.592(22.4)2=0.9922 atm.

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
Join BYJU'S Learning Program
CrossIcon