When heated, ammonium carbamate decomposes as follows
$N H_{4} C O O N H_{2} (s) ⇌ 2 N H_{3} (g) + C O_{2} (g)$
At a certain temperature, the equilibrium pressure of the system is 0.318 atm, $K_{p}$ for the reaction is

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N H 4 C O O N H 2 ( s ) E q . p r e s s u r e ⇌ 2 N H 3 ( g ) 2 P + C O 2 ( g ) P 3 P = 0.318 P = 0.106 P N H 3 = 2 × 0.106 = 0.212 P C O 2 = 0.106 k p = P N H 3 2 . P C O 2 = 0.212 × 0.212 × 0.106 = 0.00476 = 4.76 × 1 0 - 3

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