I, IV and V only
005 10.0 points
When a chemical reaction comes to equilibrium, both the forward and the reverse reactions continue, but their rates are equal. For such a system at equilibrium at 300 K and 1.00 atm pressure, the change in Gibbs free
energy as the forward reaction occurs must be
1. a maximum.
2. zero.
3. negative.
4. a minimum.
5. positive.
What is delta G at equilibrium?
I think that's what I'm looking for.
Isn't delta G at equilibrium zero?
thanks
To determine the change in Gibbs free energy (ΔG) as the forward reaction occurs at equilibrium, we need to consider the equation:
ΔG = ΔH - TΔS
where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.
For a reaction at equilibrium, the forward and reverse reactions have equal rates. This means that there is no net change in the concentrations of the reactants and products over time. Consequently, ΔG for the system at equilibrium is zero.
Therefore, the answer is 2. zero. The change in Gibbs free energy as the forward reaction occurs at equilibrium is zero because the reaction has reached a state where there is no further driving force for it to proceed in either direction.