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.
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To calculate the change in Gibbs Energy (ΔG) at a given temperature, you can use the equation:
ΔG = ΔG° + RT ln(Q)
Where:
ΔG = change in Gibbs Energy
ΔG° = standard Gibbs Energy change
R = gas constant (8.314 J/(mol*K))
T = temperature (in Kelvin)
Q = reaction quotient
In this specific case, where all product and reactant concentrations (pressures) are 1 M (1 atm) and the temperature is 298 K, the reaction quotient (Q) would equal 1.
Therefore, the equation that can be used to calculate ΔG is:
ΔG = ΔG° + (RT)ln(1)
Since ln(1) equals 0, the equation simplifies to:
ΔG = ΔG°
Thus, the correct equation to calculate ΔG in this specific scenario is:
ΔG = ΔG°
To calculate the change in Gibbs Energy (ΔG) using the available standard Gibbs Free Energy (ΔG°) values at 298 K, we can use the equation:
ΔG = ΔG° + RT ln(Q)
where:
- ΔG is the change in Gibbs Energy
- ΔG° is the standard Gibbs Free Energy at standard conditions (1 M concentrations)
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin (298 K)
- Q is the reaction quotient, which is the ratio of the product concentrations (pressures) and reactant concentrations (pressures)
Since the problem states that all product and reactant concentrations are 1 M (1 atm) at 298 K, the reaction quotient (Q) is equal to 1. Therefore, the equation simplifies to:
ΔG = ΔG°
We can see that the change in Gibbs Energy (ΔG) is equal to the standard Gibbs Free Energy (ΔG°). Thus, the equation we can use to calculate the change in Gibbs Energy in this specific case is:
ΔG = ΔG°
Therefore, the correct equation to calculate the change in Gibbs Energy is:
ΔG = ΔG°