Statement-1 : The third law of thermodynamics implies that absolute zero cannot be reached.
Statement-2 : `Delta G^(@)` for an ideal gas reaction is a function of temperature.
Statement-3 : The adiabatic expansion of a gas into a vacuum is spontaneous.

Options

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

Answer

To analyze the statements given in the question, we will evaluate each statement one by one to determine their validity.

### Step-by-Step Solution:

**Step 1: Evaluate Statement 1**
- **Statement 1:** The third law of thermodynamics implies that absolute zero cannot be reached.
- **Explanation:** The third law of thermodynamics states that as the temperature of a system approaches absolute zero (0 Kelvin), the entropy of a perfect crystal approaches zero. However, it also implies that it is impossible to reach absolute zero in a finite number of steps. Therefore, this statement is **True**.

**Step 2: Evaluate Statement 2**
- **Statement 2:** ΔG° for an ideal gas reaction is a function of temperature.
- **Explanation:** The Gibbs free energy change (ΔG) for a reaction is indeed a function of temperature, pressure, and the number of moles of reactants and products. The relationship can be expressed as ΔG = ΔH - TΔS. Since ΔH and ΔS can depend on temperature, ΔG° is also a function of temperature. Thus, this statement is **True**.

**Step 3: Evaluate Statement 3**
- **Statement 3:** The adiabatic expansion of a gas into a vacuum is spontaneous.
- **Explanation:** In an adiabatic expansion, a gas expands into a vacuum (free expansion). Since there is no opposing pressure (the vacuum has zero pressure), the gas will spontaneously expand to fill the available volume. This process does not require any energy input and occurs naturally. Therefore, this statement is **True**.

### Conclusion:
All three statements are true. Thus, the answer is **True, True, True**.

### Final Answer:
The answer is **B** (True, True, True).

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