Which of the following is incorrect

Options

A. When `DeltaGlt0` process is spontaneous
B. When `DeltaGgt0` process is non spontaneous
C. when `DeltaG=0` process is at equilibrium
D. When `DeltaGgt0` process is spontaneous

Answer

To determine which statement is incorrect regarding Gibbs free energy (ΔG), we need to analyze the relationship between ΔG, enthalpy (ΔH), entropy (ΔS), and temperature (T).

### Step-by-Step Solution:

1. **Understanding Gibbs Free Energy**:
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

2. **Interpreting ΔG Values**:
- If ΔG < 0 (negative), the process is **spontaneous**.
- If ΔG > 0 (positive), the process is **non-spontaneous**.
- If ΔG = 0, the system is at **equilibrium**.

3. **Analyzing the Statements**:
We need to identify which statement contradicts the established principles of Gibbs free energy. The key points to remember are:
- A positive ΔG indicates a non-spontaneous process.
- A negative ΔG indicates a spontaneous process.
- A ΔG of zero indicates equilibrium.

4. **Identifying the Incorrect Statement**:
Based on the principles outlined, if any statement claims that a positive ΔG corresponds to a spontaneous process, that statement would be incorrect.

5. **Conclusion**:
Therefore, the incorrect statement among the options provided is the one that states that ΔG is positive and the process is spontaneous. This is contradictory to the established rules of thermodynamics.

### Final Answer:
The incorrect statement is: "ΔG is positive and the process is spontaneous."

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