Greenhouse gas `CO_(2)` can be converted to `CO(g)` by the following reaction
`CO_(2)(g)+H_(2)(g) rarr CO_(2)+H_(2)O(g)` , termed as water gas reaction.
Based on your answer in 3,4 mark the correct box:
(a) `K_(p)` will increase with increase in temperature
(b) `K_(p)` will not change with increase in temperature
(c) `K_(p)` will decrease with increase in temperature

Answer

To determine how the equilibrium constant \( K_p \) changes with temperature for the reaction:

\[ \text{CO}_2(g) + \text{H}_2(g) \rightleftharpoons \text{CO}(g) + \text{H}_2\text{O}(g) \]

we need to analyze the nature of the reaction.

### Step 1: Identify the reaction type
This reaction is an endothermic reaction because it involves the conversion of reactants (CO2 and H2) into products (CO and H2O) with the absorption of heat.

### Step 2: Apply Le Chatelier's Principle
According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in temperature, the equilibrium will shift in a direction that counteracts the change. For endothermic reactions, increasing the temperature shifts the equilibrium to the right, favoring the formation of products.

### Step 3: Analyze the effect on \( K_p \)
As the equilibrium shifts towards the products when the temperature is increased, the concentration of the products (CO and H2O) will increase relative to the reactants (CO2 and H2). This results in an increase in the equilibrium constant \( K_p \).

### Conclusion
Thus, we conclude that:

- \( K_p \) will increase with an increase in temperature.

### Final Answer
The correct option is (a) \( K_p \) will increase with increase in temperature.

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