In a chemical reaction, `Delta H = 150 kJ and Delta S = 100 JK^(-1)` at 300 K. Therefore, `Delta`G will be

Options

A. Zero
B. 300 kJ
C. 330 kJ
D. 120 kJ

Answer

To calculate the Gibbs free energy change (ΔG) for the given reaction, we will use the formula:

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

### Step 1: Identify the given values
- ΔH = 150 kJ
- ΔS = 100 J/K
- T = 300 K

### Step 2: Convert ΔH to the same unit as ΔS
Since ΔH is given in kilojoules and ΔS is in joules, we need to convert ΔH to joules for consistency.

\[ \Delta H = 150 \text{ kJ} = 150 \times 1000 \text{ J} = 150000 \text{ J} \]

### Step 3: Substitute the values into the Gibbs free energy equation
Now we can substitute the values into the equation:

\[ \Delta G = 150000 \text{ J} - (300 \text{ K} \times 100 \text{ J/K}) \]

### Step 4: Calculate TΔS
Calculate the product of T and ΔS:

\[ T \Delta S = 300 \text{ K} \times 100 \text{ J/K} = 30000 \text{ J} \]

### Step 5: Calculate ΔG
Now substitute this value back into the equation for ΔG:

\[ \Delta G = 150000 \text{ J} - 30000 \text{ J} = 120000 \text{ J} \]

### Step 6: Convert ΔG back to kilojoules
Convert ΔG back to kilojoules:

\[ \Delta G = \frac{120000 \text{ J}}{1000} = 120 \text{ kJ} \]

### Final Answer
Thus, the change in Gibbs free energy (ΔG) is:

\[ \Delta G = 120 \text{ kJ} \]