One mole of `N_(2)O(g)` at `300K` 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 of `NO_(2)(g)`. The resultant pressure

Options

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

Answer

B

Explanation

For the given equation `N_2O_(4(g)) hArr2NO_(2(g))`
`{:("Initial",1,0),("no. of moles",,),("No. of moles", (1 – 0.2) ,0.4),("at equilibrium",,):}`
Total number of moles at equilibrium = 1.2 Initially, `P_(1) V =n_(1)RT_(1) "or " 1 xx V = 1 xx RT_(1) " or " V=RT_1`
At equilibrium `P_2V =n_(2)RT_2`
or `P_2=(1.2)/VRT_2=(1.2)/(RT_1)=(1.2)/(RT_2)=(1.2xx600)/300=2.4 atm`