One mole of `N_(2)O_(4)(g)` at 300 K is kept in a closed container under one atmosphere. It is heated to 600K when 20% by mass of `N_(2)O_(4)`(g) decomposes to `NO_(2)`(g). The resultant pressure is:

Options

A. 1.2 atm
B. 2.4 atm
C. 2.0 atm
D. 1.0 atm

Answer

B

Explanation

`{:(,N_(2)O_(4)(g), hArr, 2NO_(2)(g)),("Initially", 1,,0),("At equi.",(1-x),,2x):}`
Total mole at equilibrium `=1+x=1.2 " " therefore x=0.2`
`therefore (P_(1))/(n_(1)T_(1))=(P_(2))/(n_(2)T_(2)), (1)/(1xx300)=(P_(2))/(1.2xx600) or P_(2)=2.4` atm