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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

`4.2`

B

`5.2`

C

`3.2`

D

`6.2`

Text Solution

AI Generated Solution

To solve the problem step by step, we will analyze the decomposition of \(N_2O_4\) into \(NO_2\) and calculate the resultant pressure after the decomposition at the new temperature. ### Step 1: Understand the decomposition reaction The decomposition of \(N_2O_4\) can be represented as: \[ N_2O_4(g) \rightleftharpoons 2NO_2(g) \] From the reaction, we can see that 1 mole of \(N_2O_4\) produces 2 moles of \(NO_2\). ...
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