Question

Calculate the standard change in Gibbs free energy, ΔG'm, for the following reaction at 25.0 ℃ Standard Gibbs free energy of formation values can be found here. NH,CI(s) 근 NH, (aq) + Cl (aq) Number k.J/mol Then, determine the concentration of NH4 (aq) if the change in Gibbs free energy, AGrxn, for the reaction is-9.53 kJ/mol. Number

Answer 1

Stan dard free energy change of the reacti on,AG9.53 kJ/mol =-9.53×103 J/mol Temperature,T 25°C273 298K Gas constant, R 8.3145 JK-1mol-1 Stan dard free energy change of the reacti on, AG RTIn K In K- -9.53x10 J/mol 83145 JK"mol-1 × 298 K - 3.85 Equilibrium constant, K3846.8 Equilibrium equation is as follows: Equilibrium constant, KNH Since NH,Cl is a soli d, we can take its concentrati on as unity and exclude it from the equilibrium constant expression The ICE table I(M) 0 c(M) 0 E(M) 0 Equilibrium constant, Kea - NH Cl 46.8 = (x) (x) = x2 x 6.84 According to ICE table Concentration of NH;' | NHỊ,-(x) M - 6.84 M