Question

The decomposition of solid ammonium carbamate, `(NH_(4))(NH_(2)CO_(2))`, to gaseous ammonia and carbon dioxide is an endothermic reaction.
`9NH_(4))(NH_(2)CO_(2)))(s)hArr2NH_(3)(g)+CO_(2)(g)`
(a) When solid `(NH_(4))(NH_(2)CO_(2))` is introduced into and evacuated flask at `25^(@)C`, the total pressure of gas at equilibrium is `0.3` atm. What is the value of `K_(p) "at" 25^(@)C`?
(b) Given that the decomposition reaction is at equilibrium. how would the following changes affect the total quatity of `NH_(3)` in the flask once equilibrium is re-established?
(i) Adding `CO_(2)` (ii) Adding `(NH_(4))(NH_(2)CO_(2))`
(iii) Removing `CO_(2)` (iv) Increasing the total volume
(v) Adding neon (vi) Increasing the temperature

Answer 1

Correct Answer - (a) `2.31xx10^(-4)` (b) (i) decrease (ii) no change (iii) increase (iv) increase (v) no change (vi) increase
`(NH_(4))(NH_(2)CO_(2))(S)hArr2NH_(3)(g)+CO_(2)(g)`
2P P
Total pressure`=2P+P=0.3`
`P=0.1`atm
`K_(P)=(2P)^(2)P=4P^(3)`
`=4xx10^(-3) atm^(3)`