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From the information on deltafH and deltafG , provided in the data section calculate the standard...

From the information on deltafH and deltafG , provided in the data section calculate the standard Gibbs energy of reaction, deltarG , and the equilibrium constant, K, at: (a) 25 °C and (b) 50 °C for the chemical reaction: CH4(g) + 3 Cl2(g) -><-CHCl3 (l) + 3 HCl (g). Assume that the reaction enthalpy is independent of temperature.

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Answer #1

CH4(g) + 3Cl2(g) --------------- CHCl3(l) + 3 HCl(g)

G0rxn =[ G0f of CHCl3 + 3 xG0f of HCl] - [ G0f of CH4+3xG0f of Cl2]

G0rxn = [- 73.66 + 3x(-95.31)] - [ (-50.84)+3x0.0]

G0rxn = - 308.75KJ

Gibbs free energy change = G0 = - 308.75KJ

a) at 25C

T= 25+273= 298K

G0rxn = - RTlnK

R= 8.314x10^-3KJ

- 308.75 = - 8.314x10^-3 x298xlnK

lnK = 124.62

K = e^124.62

K= 1.32x10^54.

b) at 50C

T= 50+273= 323K

- 308.75 = - 8.314x10^-3 x323xlnK

lnK = 114.97

K= e^114.97

K= 8.53x10^49.

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