STATEMENT-1 Net reaction can occur only if a system is in equlibrium.
STATEMENT-2: All reactin tends to be in a state of equlibrium.
STATEMENT-3: At equlibrium, `DeltaG` is zero.

Options

A. T T F
B. F T T
C. T T T
D. F T F

Answer

To analyze the statements provided in the question, we will evaluate each statement one by one and determine their validity based on the principles of chemical equilibrium.

### Step-by-Step Solution:

**Step 1: Evaluate Statement 1**
- **Statement 1:** "Net reaction can occur only if a system is in equilibrium."
- **Analysis:** This statement is **false**. A net reaction can occur when a system is not in equilibrium. In fact, reactions proceed toward equilibrium, and it is during this process that the net change occurs. Once equilibrium is reached, the concentrations of reactants and products remain constant, and there is no net change in the system.

**Step 2: Evaluate Statement 2**
- **Statement 2:** "All reactions tend to be in a state of equilibrium."
- **Analysis:** This statement is **true**. Most chemical reactions do tend to reach a state of equilibrium where the rate of the forward reaction equals the rate of the reverse reaction. This is a fundamental concept in chemical kinetics and equilibrium.

**Step 3: Evaluate Statement 3**
- **Statement 3:** "At equilibrium, ΔG is zero."
- **Analysis:** This statement is **true**. At equilibrium, the Gibbs free energy change (ΔG) for the system is zero. This indicates that there is no net change in the system, and the reaction is at a state of balance. If ΔG is negative, the reaction is spontaneous in the forward direction, and if ΔG is positive, the reaction is non-spontaneous.

### Conclusion:
- **Statement 1:** False
- **Statement 2:** True
- **Statement 3:** True

### Final Answer:
- Statement 1 is false, while Statements 2 and 3 are true.

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