Which of the following statements regarding Gibb's energy change is correct?

Options

A. If `DeltaG` is negative (lt 0), the process is non-spontaneous.
B. If `DeltaG` is positive ( gt 0), the processis spontaneous.
C. If `DeltaG` is negative ( lt 0), the process is spontaneous.
D. If `DeltaG` is positive (gt 0), the process is in equilibrium.

Answer

To determine which statement regarding Gibbs energy change is correct, we will analyze the Gibbs free energy equation and the implications of its values.

### Step 1: Understand the Gibbs Free Energy Equation
The Gibbs free energy change (ΔG) is given by the equation:
\[ \Delta G = \Delta H - T \Delta S \]
where:
- ΔG = change in Gibbs free energy
- ΔH = change in enthalpy
- T = temperature in Kelvin
- ΔS = change in entropy

### Step 2: Analyze the Conditions for Spontaneity
- A process is **spontaneous** if ΔG is **negative** (ΔG < 0).
- A process is **non-spontaneous** if ΔG is **positive** (ΔG > 0).
- At **equilibrium**, ΔG is equal to **zero** (ΔG = 0).

### Step 3: Evaluate the Statements
Now, let's evaluate the given statements regarding ΔG:
1. If ΔG is negative, the process is non-spontaneous. **(Incorrect)**
2. If ΔG is positive, the process is spontaneous. **(Incorrect)**
3. If ΔG is negative, the process is spontaneous. **(Correct)**
4. For equilibrium, ΔG must be equal to 0. **(Correct)**

### Conclusion
From the analysis, the correct statements regarding Gibbs energy change are:
- If ΔG is negative, the process is spontaneous.
- For equilibrium, ΔG must be equal to 0.

Thus, the correct answer is option C: "If ΔG is negative, the process is spontaneous."