Question

In: Chemistry

From information in the “Data section” of your textbook, calculate the standard Gibbs free energy and...

From information in the “Data section” of your textbook, calculate the standard

Gibbs free energy and the equilibrium constant at (a) 25°C and (b) 50°C for the reaction

CH4(g) + 3 Cl2(g) <--> CHCl3(l) + 3 HCl (g).

Assume that the reactionenthalpy isindependent of temperature.

ΔG°f (CHCl3, l) =-­71.8 kJ/mol, ΔH°f(CHCl3, l) =‐132.2 kJ/mol

Which extra DATA can i provide from the textbook. What values should I look for?

Solutions

Expert Solution

For the given reaction,

dGo at (a) 25 oC + 273 = 298 K

dGo = dGo(products) - dGo(reactants)

        = (-71.8 + 3 x -95.31) - (-50.84 + 3 x 0)

        = -306.9 kJ/mol

dGo = -RTlnK

equilibrium constant (K)

-306.9 x 10^3 J/mol = - 8.314 x 298 lnK

K = 6.26 x 10^53

(b) at T = 50 oC + 273 = 323 K

dHo = dHo(products) - dHo(reactants)

        = (-132.2 + 3 x -92.30) - (-75 + 3 x 0)

        = -334.1 kJ/mol

dSo = dSo(products) - dSo(reactants)

        = (201.7 + 3 x 187) - (186.3 + 3 x 223)

        = -92.6 J/K.mol

dGo = dHo - TdSo

        = -334.1 - 323 x -0.0926

        = -304.2 kJ/mol

dGo = -RTlnK

equilibrium constant (K)

-304.2 x 10^3 J/mol = - 8.314 x 323 lnK

K = 1.57 x 10^49

check the values of standard dHo, dSo and dGo and reconfirm your results.


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