Ammonium carbamate dissociates on heating as:
`NH_(2)COONH_(4)(g)hArr2NH_(3)(g)+CO_(2)(g)`
The equilibrium constant `K_(p)` for the reaction, at some temperature is `3.2xx10^(-5)atm^(3)`. Calculate the partial pressure of `NH_(3)` in the equilibrium system at the same temperature.

Options

A. `2.0xx10^(-2)atm`
B. `4,0xx10^(-2)atm`
C. `3.2xx10^(-2)atm`
D. `6.4xx10^(-2)` atm

Answer

B

Explanation

`NH_(2)COONH_(4)(s)hArrunderset(2p)(2NH_(3)(g))+underset(p)(CO_(2)(g))`
`K_(p)=P_(NH_(3))^(2)xxp_(CO_(2))=(2p)^(2)xx=3.2xx10^(-5)atm^(3)`
`impliesp=2xx10^(-2)atm," "p_(NH_(3))=2xx2xx10^(-2)atm`