CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

One mole of NH4Cl(s) is kept in an open container & then covered with a lid. The container is now heated up to 600K where NH4Cl(s) completely dissociates into NH3(g) & HCl(g). If a volume of the container is 24.63 liters, calculate what will be the final pressure of the gases inside the container? Assume that outside air is at 300K and 1 atm pressure.

A
0.5 atm;
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
2.5 atm;
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
1.5 atm;
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
None of these
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
Open in App
Solution

The correct option is D None of these
NH4Cl(s)1 molNH3(g)1 mol+HCl(g)1 mol

P=nRTV=2×0.0821×60024.63=4atm

Thus, the total pressure of gases inside container is 4 atm.

flag
Suggest Corrections
thumbs-up
0
similar_icon
Similar questions
View More
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Mole Concept
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon