A change in the free energy of a system at constant temperature and pressure will be:
`Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S`
At constant temperature and pressure
`Delta_(sys) G lt 0` (spontaneous)
`Delta_(sys)G = 0` (equilibrium)
`Delta_(sys)G gt 0` (non-spontaneous)
For a spontaneous reaction `DeltaG`, equilibrium `K` and `E_(cell)^(Theta)` will be, respectively

Options

A. `-ve, gt 1, +ve`
B. `-ve, lt1, -ve`
C. `+ve, gt1, -ve`
D. `-ve, gt1, -ve`

Explanation

To solve the problem regarding the values of ΔG, K, and E°cell for a spontaneous reaction, we can follow these steps:

### Step 1: Understand the Gibbs Free Energy Change (ΔG)
The Gibbs free energy change (ΔG) indicates whether a reaction is spontaneous or not. For a spontaneous reaction, ΔG must be negative.

**Hint:** Recall that a negative ΔG indicates that the products are more stable than the reactants, making the reaction favorable.

### Step 2: Relationship Between ΔG and the Equilibrium Constant (K)
...