According to Le-Chatelier’s principle, the increase of temperature in the following reaction
`CO_(2)(g) + 2H_(2)O(g) rarr CH_(4)(g) + 2O_(2)(g)`
will cause it shift to the right. This reaction is, therefore :

Options

A. Exothermic
B. Unimolecular
C. Endothermic
D. Spontaneous

Explanation

To solve the question regarding the effect of temperature on the given reaction according to Le Chatelier's principle, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction**: The reaction given is:
\[ CO_2(g) + 2H_2O(g) \rightleftharpoons CH_4(g) + 2O_2(g) \]

2. **Understand Le Chatelier's Principle**: Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change and restore a new equilibrium.

3. **Analyze the Effect of Temperature**: The question states that increasing the temperature will cause the reaction to shift to the right. This implies that the products (CH₄ and O₂) are favored at higher temperatures.

4. **Determine the Type of Reaction**:
- In an endothermic reaction, heat is absorbed, and increasing the temperature shifts the equilibrium to the right (toward products).
- In an exothermic reaction, heat is released, and increasing the temperature shifts the equilibrium to the left (toward reactants).

5. **Conclude the Nature of the Reaction**: Since the equilibrium shifts to the right with an increase in temperature, the reaction must be endothermic. This means that heat can be considered as a reactant, and the reaction absorbs heat.

6. **Final Answer**: Therefore, the reaction is an **endothermic reaction**.