Which of the following statement is/are false ?

Options

A. `Delta_rS` for `1/2Cl_2(g)toCl(g)` is positive
B. `DeltaElt0` for combustion of `CH_4(g)` in a sealed container with rigid adiabatic system
C. `DeltaG` is always zero for a reversible process in a closed system
D. `DeltaG^@` for an ideal gas reaction is a function of pressure

Explanation

To determine which statements are false, we will evaluate each statement one by one.

### Step 1: Analyze Statement A
**Statement A:** Delta S (entropy change) is positive for the conversion of Cl2 gas to Cl gas.

- **Analysis:** When Cl2 gas dissociates into 2 Cl gas atoms, the number of gas molecules increases, which leads to an increase in randomness or disorder. Therefore, the change in entropy (ΔS) is indeed positive.

**Conclusion:** This statement is true.

### Step 2: Analyze Statement B
**Statement B:** Delta E (change in internal energy) is negative for the combustion of methane in a sealed container with a rigid adiabatic system.

- **Analysis:** In a sealed container with no volume change (rigid), the work done (W) is zero (since W = PΔV and ΔV = 0). In an adiabatic system, there is no heat exchange (Q = 0). Therefore, ΔE = Q + W = 0 + 0 = 0, not negative.

**Conclusion:** This statement is false.

### Step 3: Analyze Statement C
**Statement C:** Delta G (Gibbs free energy) is always 0 for a reversible process in a closed system.

- **Analysis:** Delta G is equal to zero only at equilibrium. For a reversible process, the system is not necessarily at equilibrium throughout the process. Therefore, this statement is incorrect.

**Conclusion:** This statement is false.

### Step 4: Analyze Statement D
**Statement D:** Delta G0 (standard Gibbs free energy change) for an ideal gas reaction is a function of pressure.

- **Analysis:** The standard Gibbs free energy change (ΔG0) is related to the reaction's equilibrium constant (K) and is not directly a function of pressure. It is defined under standard conditions, and while ΔG can change with pressure, ΔG0 itself is constant for a given reaction at a specific temperature.

**Conclusion:** This statement is false.

### Final Conclusion
The false statements are:
- Statement B: Delta E is negative for combustion of methane in a sealed container with a rigid adiabatic system.
- Statement C: Delta G is always 0 for a reversible process in a closed system.
- Statement D: Delta G0 for an ideal gas reaction is a function of pressure.

### Summary of False Statements
- **False Statements:** B, C, and D.

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