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)
The free enegry for a reaction having `DeltaH = 31400 cal, DeltaS = 32 cal K^(-1) mol^(-1) at 1000^(@)C` is

Options

A. `-9336 cal`
B. `-7006 cal`
C. `-2936 cal`
D. `+9006 cal`

Explanation

To solve the problem, we need to calculate the Gibbs free energy change (ΔG) using the given formula:

\[ \Delta G = \Delta H - T \Delta S \]

### Step 1: Identify the given values
- ΔH = 31400 cal
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