Suppose the ÄGof, ÄHof, and ÄSo 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.
ÄG=ÄGo+RT ln Q
ÄGo=ÓÄGof(products)- ÓÄGof(reactants)
ÄGo=ÄHo-TÄSo
ÄGo= -RT ln K
I can only guess as to the meaning of some of the symbols. Assuming my guesses are right, and I don't guarantee they are, I would go with B followed by A.
To determine the equation(s) that can be used to calculate the change in Gibbs Energy (ΔG) under the given conditions, we need to consider the formulas related to Gibbs Energy (G), enthalpy (H), entropy (S), and the equilibrium constant (K).
The correct equation(s) to calculate ΔG in this scenario are:
1. ΔG = ΔGo + RT ln Q
This equation is the standard equation for calculating the change in Gibbs Energy using the standard Gibbs Energy of formation (ΔGof) for the products and reactants, gas constant (R), temperature (T), and the reaction quotient (Q).
2. ΔGo = ΣΔGof(products) - ΣΔGof(reactants)
This equation is used to calculate the standard Gibbs Energy change (ΔGo) by subtracting the sum of the standard Gibbs Energy of formation (ΔGof) of the reactants from the sum of the ΔGof of the products.
3. ΔGo = ΔHo - TΔSo
This equation relates the change in Gibbs Energy with the change in enthalpy (ΔH) and the change in entropy (ΔS), where T is the temperature in Kelvin.
4. ΔGo = -RT ln K
This equation is based on the relationship between the equilibrium constant (K) and the Gibbs Energy change (ΔG). It uses the gas constant (R), temperature (T), and the natural logarithm (ln) of the equilibrium constant.
Therefore, options 1, 2, and 4 could be used to calculate the change in Gibbs Energy in this situation.