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 pressureA. `1.2 atm`B. 2.4 atmC. `2.0` atmD. `1.0` atm

One mole of `N_(2)O(g)` at `300K` is kept in a closed container under

1.	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 pressureA. `1.2 atm`B. 2.4 atmC. `2.0` atmD. `1.0` atm
Answer» Correct Answer - B `N_(2)O_(4)(g) hArr 2NO_(2)(g)` At start `=100 // 92 mol = 1.08 mol ` 0 At equilibrium `80 // 92 mol = 0.86` `20 // 46 mol = 0.43 mol` According to ideal gas equation, at two condition At 300 K `P_(0)V=n_(0)RT_(0)` `1 xx V = 1.08 xx R xx300` ....(i ) At 600K `P_(1)V = n_(2)RT_(1)` `P_(1)xxV = (0.86+0.43) xx R xx 600` ....(ii) Divide (ii) by (i) `(P_(1))/(1) = (1.29xx600)/(1.08xx300), P_(1)= (1.29xx2)/(1.08) = 2.38 atm`.

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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 pressureA. `1.2 atm`B. 2.4 atmC. `2.0` atmD. `1.0` atm

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