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A mixture of 3 mol Cl2 and 3 mol of co is enclosed in a 5l flask at 600 degrees c. When the reaction reaches equilibrium, only 3.30% of the cl2 has been consumed. Calculate the delta g for the reaction at this temperature?
Accepted Answer
The equilibrium constant for the reaction is given by:
K = [CO2][Cl2] / [CO][Cl2]^2
We can use the equilibrium constant to calculate the Gibbs free energy change for the reaction:
ΔG° = -RTlnK
where R is the gas constant (8.314 J/mol·K) and T is the temperature in Kelvin (600 K).
We can substitute the equilibrium constant and temperature into the equation to calculate the Gibbs free energy change:
ΔG° = -8.314 J/mol·K * 600 K * ln(0.033)
ΔG° = 12.8 kJ/mol
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