Calculate the free energy change, delta G, for the reaction at 150C Cl2 (g) + CO

Question

Calculate the free energy change, delta G, for the reaction at 150C Cl2 (g) + CO (g) --> COCl2 (g) Given the following thermodynamic data:
Substance delta H (kJ/mol) S(J/mol* K) Cl2 (g) 0.00 223 CO (g) -110 198 COCl2 (g) -219 289

A. -53.2 kJ B. -88.3 kJ C. -108 kJ D. 131 kJ E. 88.8 kJ Cl2 (g) + CO (g) --> COCl2 (g) Given the following thermodynamic data:
Substance delta H (kJ/mol) S(J/mol* K) Cl2 (g) 0.00 223 CO (g) -110 198 COCl2 (g) -219 289

A. -53.2 kJ B. -88.3 kJ C. -108 kJ D. 131 kJ E. 88.8 kJ

Explanation / Answer

We Know that         According togibb's equation :         G = H - T S                           H = Hproducts - Hreactants                   = -109 x 103 J           S = Sproducts - Sreactants                  = -132 J / K          T = 1500C   = 423 K        Substituting the valuesin the equation :            G = -109 x 103 J - 423 Kx - 132 J / K                    = - 53164 J                    = - 53. 2 KJ   option A is correct.                  = -132 J / K          T = 1500C   = 423 K        Substituting the valuesin the equation :            G = -109 x 103 J - 423 Kx - 132 J / K                    = - 53164 J                    = - 53. 2 KJ   option A is correct.

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