Which of the following reactions of hydrogen with non - metals represents Haber's process ?

Options

A. `2H_(2) + O_(2) overset("heat")rarr 2H_(2) O, Delta H = -285.9 "kj mol"^(-1)`
B. `3H_(2)+N_(2)overset(673 K, Fe)underset(200 atm)rarr 2NH_(3), Delta H=-92.6 "kJ mol"^(-1)`
C. `H_(2) + Cl_(2) overset(hv)rarr 2HCI`
D. `2H_(2) + C overset(1100^(@)C)rarr CH_(4)`

Explanation

To determine which reaction represents Haber's process, we need to understand what Haber's process is. Haber's process is the synthesis of ammonia (NH3) from nitrogen gas (N2) and hydrogen gas (H2). The balanced chemical equation for this process is:

\[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \]

Now, let's analyze the given options step by step:

1. **Option A: \( H_2 + O_2 \rightarrow H_2O \)**
- This reaction represents the formation of water (H2O) from hydrogen and oxygen. This does not represent Haber's process.

2. **Option B: \( H_2 + N_2 \rightarrow NH_3 \)**
- This reaction shows hydrogen reacting with nitrogen to produce ammonia (NH3). This is indeed the essence of Haber's process, although the balanced equation would require three moles of hydrogen for every mole of nitrogen to produce two moles of ammonia. Thus, this option represents Haber's process.

3. **Option C: \( H_2 + Cl_2 \rightarrow HCl \)**
- This reaction represents the formation of hydrogen chloride (HCl) from hydrogen and chlorine. This does not represent Haber's process.

4. **Option D: \( H_2 + CH_4 \rightarrow \) (not specified)**
- This reaction involves hydrogen and methane (CH4), but it does not produce ammonia. Therefore, it does not represent Haber's process.

After analyzing all the options, we conclude that the reaction that represents Haber's process is:

**Answer: Option B: \( H_2 + N_2 \rightarrow NH_3 \)**