Calculate ΔG (in kJ) for the reaction:
CO2(g) + CCl4(g) = 2 COCl2(g)
at 25oC under the conditions:
CO2 = 0.120 atm, CCl4 = 0.162 atm, and COCl2 = 0.856 atm.
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To calculate ΔG (change in Gibbs free energy) for the given reaction, we can use the equation:
ΔG = ΔG° + RTln(Q)
Where:
ΔG is the change in Gibbs free energy
ΔG° is the standard Gibbs free energy change for the reaction at standard conditions
R is the gas constant (8.314 J/K·mol)
T is the temperature in Kelvin
ln is the natural logarithm
Q is the reaction quotient, calculated as the ratio of the partial pressures of the products to the partial pressures of the reactants.
First, we need to calculate ΔG° for the reaction. The standard Gibbs free energy change (ΔG°) can be obtained from standard Gibbs free energy values of formation of the compounds involved in the reaction. These values can be found in thermodynamic tables or databases.
Next, we need to calculate the reaction quotient (Q) by taking the partial pressures of the products and dividing it by the partial pressures of the reactants:
Q = (P(COCl2))^2 / (P(CO2) * P(CCl4))
Given that CO2 = 0.120 atm, CCl4 = 0.162 atm, and COCl2 = 0.856 atm, we can substitute these values into the equation to solve for Q:
Q = (0.856)^2 / (0.120 * 0.162)
Once we have ΔG° and Q, we can substitute them into the equation mentioned at the beginning to calculate ΔG. Remember to convert the temperature from Celsius to Kelvin (25oC = 25 + 273 = 298 K).
It is important to note that the given values of CO2, CCl4, and COCl2 are partial pressures at the given conditions. If you only have concentrations or moles, you will need to convert them to partial pressures using the ideal gas law.