Statement -1: For every chmical reaction at equilibrium , standard Gidds energy of reaction is zero
Statement-2: At constant temperature and pressure , chemical reactions are spontaneious in the direction of decreasing gibbs energy.

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
B. Statement-1 is True, Statement-2 is True, Statement-2 is not a correct explanation for Statement-1
C. Statement-1 is True, Statement-2 is false
D. Statement-1 is False, Statement-2 is True

Explanation

To analyze the statements provided in the question, we will evaluate each statement based on our understanding of Gibbs free energy and its implications for chemical reactions at equilibrium.

### Step-by-Step Solution:

1. **Understanding Gibbs Free Energy**:
- Gibbs free energy (G) is a thermodynamic potential that helps predict the direction of chemical reactions. It is defined as:
\[ G = H - TS \]
where \(H\) is enthalpy, \(T\) is temperature, and \(S\) is entropy.

2. **Standard Gibbs Free Energy**:
- The standard Gibbs free energy change (\( \Delta G^\circ \)) for a reaction is the change in Gibbs free energy when reactants are converted to products under standard conditions (1 bar pressure, 1 M concentration, and a specified temperature).
- The relationship between Gibbs free energy change and the equilibrium constant (K) is given by:
\[ \Delta G = \Delta G^\circ + RT \ln Q \]
where \(Q\) is the reaction quotient.

3. **Evaluating Statement 1**:
- Statement 1 claims that "For every chemical reaction at equilibrium, the standard Gibbs energy of reaction is zero."
- At equilibrium, the Gibbs free energy change (\( \Delta G \)) is zero, but this does not imply that the standard Gibbs free energy change (\( \Delta G^\circ \)) is also zero.
- Therefore, Statement 1 is **incorrect**.

4. **Evaluating Statement 2**:
- Statement 2 states that "At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy."
- This statement is true because a spontaneous reaction occurs when the Gibbs free energy of the system decreases (\( \Delta G < 0 \)).
- As the reaction progresses towards equilibrium, the Gibbs free energy decreases, confirming that Statement 2 is **correct**.

5. **Conclusion**:
- Based on the evaluations, Statement 1 is incorrect, and Statement 2 is correct. Therefore, the answer is that Statement 2 is true, while Statement 1 is false.

### Final Answer:
- **Statement 1**: Incorrect
- **Statement 2**: Correct