Suppose the ΔGof, ΔHof, and ΔSo are available and valid at 298 K. Which equation(s) could be used to calculate the change in Gibbs Energy if all product and reactant concentrations (pressures) are 1 M (1 atm) and the temperature is 298 K? Choose all that apply.
ΔGo=ΔHo-TΔSo
ΔG=ΔGo-RT ln Q
ΔGo= -RT ln K
ΔGo=ΣΔGof(products)- ΣΔGof(reactants)
o=Knot
To calculate the change in Gibbs Energy (ΔG) using the given information, you can use the following equations:
1. ΔGo = ΔHo - TΔSo
This equation relates the standard Gibbs Free Energy change (ΔGo) with the standard enthalpy change (ΔHo) and the standard entropy change (ΔSo).
2. ΔG = ΔGo - RT ln Q
This equation relates the actual Gibbs Free Energy change (ΔG) with the standard Gibbs Free Energy change (ΔGo), the gas constant (R), the temperature (T), and the reaction quotient (Q). Q can be calculated using the concentrations (or pressures) of the reactants and products.
3. ΔGo = -RT ln K
This equation relates the standard Gibbs Free Energy change (ΔGo) with the equilibrium constant (K) at the given temperature. K can be calculated using the concentrations (or pressures) of the reactants and products.
4. ΔGo = ΣΔGof(products) - ΣΔGof(reactants)
This equation relates the standard Gibbs Free Energy change (ΔGo) with the standard Gibbs Free Energy of formation (ΔGof) of the products and reactants. The ΔGof values are usually tabulated values.
All of these equations could be used to calculate the change in Gibbs Energy (ΔG) if all product and reactant concentrations (pressures) are 1 M (1 atm) and the temperature is 298 K.