Consider the reaction equilibrium
`underset(("Greater volume"))("Ice")hArrunderset(("Lesser volume"))("Water -xkcal")` The favourable conditions for forward reaction are

Options

A. low temperature , high pressure and excess of ice
B. low temperature , low pressure and excess of ice
C. high temperature ,low pressure and excess of ice
D. high temperature , high pressure and excess of ice

Answer

To determine the favorable conditions for the forward reaction in the equilibrium between ice and water, we can analyze the reaction step by step.

### Step 1: Understand the Reaction
The reaction is represented as:
\[ \text{Ice} \rightleftharpoons \text{Water} - x \text{kcal} \]
This indicates that ice can convert to water, and this process requires the absorption of energy (x kcal).

### Step 2: Identify the Nature of the Reaction
The conversion of ice (solid) to water (liquid) is an endothermic process, meaning it requires heat (energy) to proceed. Therefore, increasing the temperature will favor the forward reaction (ice to water).

### Step 3: Consider the Volume Change
In this reaction, ice occupies a greater volume compared to water. According to Le Chatelier’s principle, if the volume decreases (as in the case of ice melting into water), increasing the pressure will favor the forward reaction. Thus, applying high pressure will also promote the conversion of ice to water.

### Step 4: Summarize the Conditions
From the above analysis, we can conclude that the conditions that favor the forward reaction (conversion of ice to water) are:
- **High Temperature**: This provides the necessary energy for the endothermic process.
- **High Pressure**: This favors the side of the reaction with lesser volume (water).
- **Excess of Ice**: Having more ice can drive the reaction towards producing more water.

### Final Answer
The favorable conditions for the forward reaction are:
- High Temperature
- High Pressure
- Excess of Ice