Ammonium carbonate nh4co2nh2 decomposes as follows
nh4co2nh2< > 2nh3(g) + co2(g)

starting with only the solid, it is found that at 40 c the total gas pressure (nh3 and co2) is 0.463 atm. calculate the equilibrium constant kp.

Kp = 0.0146

Explanation:

We can solve this equilibrium problem using an ICE Table. There are 3 stages: I(Initial), C(Change) and E(Equilibrium). Only gases and aqueous species participate in the equilibrium.

    NH₄CO₂NH₂ ⇄ 2 NH₃(g) + CO₂(g)

I                                    0             0

C                                 +2x          +x

E                                   2x            x

Total gas pressure is equal to the sum of partial pressures at equilibrium.

pNH₃ + pCO₂ = 0.463 atm

 2x    +     x     = 0.463 atm

 3 x = 0.463 atm

    x = 0.154 atm

Then,

pNH₃ = 0.308 atm

pCO₂ = 0.154 atm

We can replace this data in the Kp expression.

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1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%