1. Using thermodynamic data given below, calculate the standard Gibbs free energy change, delta G degrees rxn, for the combustion of one mole of methane using the standard free energies of formation of the products and reactants. Is the reation product-facoured or reactant favoured at equilibrium? CH4(g) + 2O2 (g) → 2H2O(g) + CO2(g) Gibbs free energies of formation in kJ/mol at 298.15K: CH4(g) = -50.8 ; H2O(g) = - 228.6; CO2(g) = -394.4 2. Determine the standard free energy change delta G degrees rxn, for the formation of 1.00 mol of NH3(g) from nitrogen and hydrogen. Use this value to calculate the equilibrium constant for this reaction at 25 degrees C . Note that the tabulated value for delta f G degrees for NH3(g) is -16.37kJ/mol
I am having trouble understanding the following entropy questions, any guidence or help would be greatly appreciated :).
1. Using
CH4(g) + 2O2 (g) → 2H2O(g) + CO2(g)
Gibbs free energies of formation in kJ/mol at 298.15K:
CH4(g) = -50.8 ; H2O(g) = - 228.6; CO2(g) = -394.4
2. Determine the standard free energy change delta G degrees rxn, for the formation of 1.00 mol of NH3(g) from nitrogen and hydrogen. Use this value to calculate the equilibrium constant for this reaction at 25 degrees C .
Note that the tabulated value for delta f G degrees
for NH3(g) is -16.37kJ/mol
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