Question

For the reaction below, the thermodynamic equilibrium constant is K = 2.30×10−4 at 25 °C.

NH4CO2NH2(s) ⟶ 2 NH3(g) + CO2(g)

Suppose that 0.0156 moles of NH4CO2NH2, 0.0312 moles of NH3, and 0.0156 moles of CO2 are added to a 5.00 L container at 25 °C.

(a) What are Q and ΔrG (kJ mol−1) for the initial reaction mixture?

Answer 1

(NH3) = 0.0312 mols/5 L = approx 0.006
(CO2) = 0.0156 mols/5 L = approx 0.003
Note that concn NH4CO2NH2 doesn't matter since it doesn't appear in the Q expression.
NH4CO2NH2(s) ⟶ 2 NH3(g) + CO2(g)
dG = -RTlnQ
dG = -RTln(NH3)^2*(CO2)
Substitute and solve for Q and dG.
BTW, what does r stand for in delta r G?
Note that my calculations are approx. You need to recalculate all.
Also note that dG will be in joules and you will need to convert to kJ.

Answer 2

r stands for reaction! thanks for ur help