For a certain process, at 328 K, $\Delta$ G = -21.0 kJ and $\Delta$ H = -5.00 kJ. If the process is carried out in such a way that no useful work is performed, what is $\Delta$ G?

Question

Quizplus · Accepted Answer

If no useful work is performed, the change in Gibbs free energy (ΔG) is equal to the change in enthalpy (ΔH) minus the product of the temperature (T) and the change in entropy (ΔS): ΔG = ΔH - TΔS. Therefore, since ΔH is given to be -5.00 kJ and we are trying to find ΔG, we need to solve for ΔS. Rearranging the equation, we get ΔS = (ΔH - ΔG) / T. Plugging in the values given, we get ΔS = (-5.00 kJ - (-21.0 kJ)) / 328 K = 0.488 kJ/K. Now we can use the equation ΔG = ΔH - TΔS to solve for ΔG: ΔG = -5.00 kJ - (328 K)(0.488 kJ/K) = -21.0 kJ. Therefore, the answer is E, -21.0 kJ.

For a Certain Process, at 328 K Δ\DeltaΔ G = -210 KJ And Process

For a Certain Process, at 328 K $\Delta$ G = -210 KJ And Process