What is the sign of `Delta G` for the process of ice melting at 283 K ?

Options

A. `Delta G gt 0`
B. `Delta G = 0`
C. `Delta G lt 0`
D. None of these

Explanation

To determine the sign of ΔG (Gibbs free energy change) for the process of ice melting at 283 K, we can follow these steps:

### Step 1: Understand the process
The process in question is the melting of ice (solid H2O) into liquid water (H2O). This phase change occurs at a specific temperature known as the melting point.

### Step 2: Identify the melting point
The melting point of ice is 273 K. At this temperature, ice and liquid water are in equilibrium.

### Step 3: Analyze the temperature given
The temperature given in the question is 283 K, which is above the melting point of ice (273 K).

### Step 4: Apply the Gibbs free energy equation
The Gibbs free energy change (ΔG) for a process can be related to the temperature and the enthalpy (ΔH) and entropy (ΔS) changes of the process using the equation:
\[ \Delta G = \Delta H - T \Delta S \]

### Step 5: Determine the signs of ΔH and ΔS
- For the melting of ice:
- ΔH (enthalpy change) is positive because energy is absorbed to break the bonds in the solid state.
- ΔS (entropy change) is also positive because the disorder increases when ice melts into liquid water.

### Step 6: Evaluate ΔG at 283 K
Since the temperature (283 K) is above the melting point (273 K), the process of melting ice is spontaneous. In this case, ΔG will be negative:
- The positive ΔS term (increased disorder) will outweigh the positive ΔH term (energy absorbed) at this temperature.

### Conclusion
Therefore, at 283 K, the sign of ΔG for the melting of ice is negative (ΔG < 0).

### Final Answer
The sign of ΔG for the process of ice melting at 283 K is negative.

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