Statement-1: A reaction which is spontaneous and accompained by decrease of randomness must be exothermic.
Statement -2: All exothermic reaction that are accomained by decrease of randomness.

Options

A. If both the statements are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-10
B. If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-10
C. If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To analyze the statements provided in the question, we will break down the concepts of spontaneity, enthalpy, and entropy step by step.

### Step-by-Step Solution:

1. **Understanding Spontaneity**:
- A reaction is considered spontaneous if it occurs without needing to be driven by an external force. For a reaction to be spontaneous, the change in Gibbs free energy (ΔG) must be negative.

2. **Gibbs Free Energy Equation**:
- The relationship between Gibbs free energy, enthalpy (ΔH), and entropy (ΔS) at a constant temperature (T) is given by the equation:
\[ \Delta G = \Delta H - T \Delta S \]

3. **Analyzing Statement 1**:
- Statement 1 claims that a reaction which is spontaneous and accompanied by a decrease in randomness (which implies a decrease in entropy, ΔS < 0) must be exothermic (ΔH < 0).
- If ΔS is negative, then -TΔS is positive (since T is always positive). Thus, the equation becomes:
\[ \Delta G = \Delta H + \text{(positive value)} \]
- For ΔG to be negative, ΔH must also be negative (ΔH < 0). This indicates that the reaction is exothermic.
- Therefore, Statement 1 is **correct**.

4. **Analyzing Statement 2**:
- Statement 2 claims that all exothermic reactions are accompanied by a decrease in randomness (ΔS < 0).
- This is not necessarily true. While some exothermic reactions may have a decrease in entropy, there are also exothermic reactions where entropy increases (ΔS > 0).
- For example, the combustion of a substance may produce more gas molecules than were present in the reactants, leading to an increase in entropy.
- Therefore, Statement 2 is **false**.

### Conclusion:
- **Statement 1** is true: A spontaneous reaction accompanied by a decrease in randomness must be exothermic.
- **Statement 2** is false: Not all exothermic reactions are accompanied by a decrease in randomness.