For a reaction to proceed

Options

A. `DeltaG` should be negative
B. `DeltaG` should be positive
C. No role of `Delta G`
D. None of the above

Answer

To determine the conditions under which a chemical reaction can proceed, we need to analyze the Gibbs free energy change (ΔG) associated with the reaction. Here’s a step-by-step solution to the question:

### Step 1: Understand the concept of Gibbs Free Energy (ΔG)
Gibbs Free Energy (ΔG) is a thermodynamic potential that helps predict whether a reaction will occur spontaneously at constant temperature and pressure.

### Step 2: Identify the conditions for spontaneity
For a reaction to be spontaneous (i.e., to proceed without external influence), the change in Gibbs Free Energy (ΔG) must be negative. This indicates that the products of the reaction have lower energy than the reactants, and thus the reaction can occur naturally.

### Step 3: Analyze the options provided
The question provides four options regarding the value of ΔG:
1. ΔG should be negative
2. ΔG should be positive
3. No role of ΔG
4. None of these

### Step 4: Determine the correct option
From our understanding of Gibbs Free Energy:
- If ΔG < 0 (negative), the reaction is spontaneous.
- If ΔG > 0 (positive), the reaction is non-spontaneous.
- If ΔG = 0, the system is at equilibrium, meaning no net change occurs.

Since we are looking for the condition under which a reaction can proceed spontaneously, the correct answer is:
**ΔG should be negative.**

### Conclusion
Thus, the correct answer to the question is option 1: **ΔG should be negative.**

---