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One "mole" of N(2)O(4)(g) at 100 K is ke...

One "mole" of `N_(2)O_(4)(g)` at `100 K` is kept in a closed container at `1.0` atm pressure. It is heated to `400 K`, where `30%` by mass of `N_(2)O_(4)(g)` decomposes to `NO_(2)(g)`. The resultant pressure will be

A

`1.2` atm

B

`2.4` atm

C

`2.0` atm

D

`1.0` atm

Text Solution

Verified by Experts

The correct Answer is:
B
`{:(N_(2)O_(4),hArr,2NO_(2)),(1,,0),((1-0.2),,2xx0.2=0.4):}`
Total pressure `=1.2`
As the temperature is doubled, the pressure becomes double. Therefore, the total final pressure is `1.2xx2=2.4` atm.
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