Which among the following reactions is favoured in forward direction by increase of temperature?

Options

A. `N_(2)(g)3H_(2)(g) hArr 2NH_(3)(g)+22.9 kcal`
B. `N_(2)(g)+O_(2)(g) hArr 2NO(g)-42.8 kcal`
C. `2SO_(2)(g)+O_(2)(g) hArr 2SO_(3)(g)+45.3 kcal`
D. `H_(2)(g)+Cl_(2)(g) hArr 2HCl(g)` `-44 kcal`

Explanation

To determine which of the given reactions is favored in the forward direction by an increase in temperature, we need to analyze the enthalpy change (ΔH) of each reaction. Here's a step-by-step solution:

### Step 1: Understand the Concept of Enthalpy Change
- Enthalpy change (ΔH) indicates whether a reaction is endothermic or exothermic.
- If ΔH > 0, the reaction is endothermic, meaning it absorbs heat.
- If ΔH < 0, the reaction is exothermic, meaning it releases heat.

### Step 2: Identify the Effect of Temperature on Reactions
- For endothermic reactions (ΔH > 0), an increase in temperature favors the forward direction of the reaction.
- For exothermic reactions (ΔH < 0), a decrease in temperature favors the forward direction of the reaction.

### Step 3: Analyze the Given Options
- We need to check the ΔH values provided for each reaction.
- We are looking for reactions with ΔH > 0 (endothermic reactions).

### Step 4: Evaluate Each Reaction
- **Option 1:** Check if ΔH > 0.
- **Option 2:** Check if ΔH > 0.
- **Option 3:** Check if ΔH > 0.
- **Option 4:** Check if ΔH > 0.

### Step 5: Identify the Correct Options
- From the analysis, if options 1 and 3 have ΔH > 0, then these reactions are favored in the forward direction with an increase in temperature.

### Conclusion
- The reactions that are favored in the forward direction by an increase in temperature are those with positive ΔH values. Therefore, the correct answers are **Option 1 and Option 3**.

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