Ammonium carbonate decomposes as N H 2 C O O N H 4 s ⇌ 2 N H 3 g + C O 2 ( g ) For the reaction, K p = 2.9 × 10 - 5 a t m 3 . If we start with 1 mole of the compound, the total pressure at equilibrium would be

Step-by-step solution

N H 2 C O O N H 4 s ⇌ 2 N H 3 g + C O 2 ( g ) At equilibrium if partial pressure of C O 2 is p then that of N H 3 is 2 p So, K p = p NH 3 2 × p CO 2 K p = 2 p 2 × p = 4 p 3 2.9 × 10 - 5 = 4 p 3 p = 1.935 × 10 - 2 hence, total pressure p = 3 p = 5.81 × 10 - 2 = 0.0581 atm.