Question

A)

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction.

2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ

P(Hg) = 0.025 atm, P(O₂) = 0.037 atm

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction.

2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ

P(Hg) = 0.025 atm, P(O₂) = 0.037 atm

-164 kJ
+60.7 kJ
+207 kJ
-26.5 kJ
-154.4 kJ B) Estimate ΔG°rxn for the following reaction at 449.0 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH°= -94.9 kJ; ΔS°= -224.2 J/K Estimate ΔG°rxn for the following reaction at 449.0 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH°= -94.9 kJ; ΔS°= -224.2 J/K +5.8 kJ -4.2 kJ -101 kJ +2.4 kJ +12.9 kJ C) Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K 2.51 × 10-13 3.99 × 1012 3.07 × 1011 3.26 × 10-12 13.0 D)
A reaction has ΔH∘rxn=−239kJ and ΔS∘rxn= 247J/K.	Part A Calculate ΔG∘rxn at 46 ∘C. Calculate at 46 . −250kJ −318kJ −7.90×104kJ −1.16×104kJ

Answer 1

A)

2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ

P(Hg) = 0.025 atm, P(O₂) = 0.037 atm

Kp = P^2 _HgO(s) / P^2 _Hg x P_O2

HgO is a solid

Kp = 1/P^2 _Hg x PO2

Kp = 1/ ( 0.025)^2x ( 0.037)

Kp = 43243.24

T= 298K            R = 8.314x10^-3 KJ

Grxn = G0rxn + RT lnKp

Grxn = - 180.8 + 8.314x10^-3 x 298 x ln(43243.24)

Grxn = - 154.35KJ

Grxn = - 154.5 KJ

B)

ΔH°= -94.9 kJ; ΔS°= -224.2 J/K

T = 449.0K

G0rxn = H0rxn - TS0rxn

G0rxn = - 94.9 - ( 449.0 x ( -224.2)]

G0rxn = + 5.76KJ

G0rxn = + 5.8 KJ

C)

HCN(g) + 2 H₂(g) → CH₃NH₂(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K

G0rxn = H0rxn - TS0rxn

G0rxn = - 158 - [ 298x ( -219.9)]

G0rxn = - 92.47 KJ

G0rxn = - RT lnK

R= 8.314x10^-3KJ       T = 655K

- 92.47 = - 8.314x10^-3 x 655 x lnK

lnK = 16.98

K = e^16.98 =

d)

ΔH∘rxn=−239kJ and ΔS∘rxn= 247J/K.

G0rxn = H0rxn - TS0rxn

T = 46C = 46+273= 319K

G0rxn = - 239 - ( 319 x 247)

G0rxn = - 317.79 Kj

G0rxn = - 318 KJ

_K