To analyze this industrial process for the production of ammonia via the Haber Process, let’s delve into the details given:
1. Reaction Equation:
[tex]\[ N_2(g) + 3 H_2(g) \rightarrow 2 NH_3(g) + 100.4 \text{ kJ} \][/tex]
2. Reaction Conditions:
- Temperature: \( 200^\circ \text{C} \)
- Pressure: \(1000 \text{ atmospheres}\)
3. Yield:
- The yield of \( NH_3 \) is approximately \( 98\% \).
4. Exothermic Reaction:
- The reaction releases \( 100.4 \text{ kJ} \) of heat, indicating that it is an exothermic reaction.
Let us interpret these points step-by-step:
### 1. Reaction Type
The first thing to notice is the heat term on the product side of the reaction. The notation “+ 100.4 kJ” indicates that heat is released during the reaction. When a chemical reaction releases heat, it is classified as an exothermic reaction. Hence, this reaction is exothermic.
### 2. Yield of \( NH_3 \)
Yield refers to the efficiency of the reaction in converting reactants into products. The statement specifies that the yield for \( NH_3 \) is approximately \( 98\% \), indicating that under the given conditions, you will obtain \(98\% \) of the theoretically calculated amount of \( NH_3 \).
### 3. Ideal Conditions for the Yield
- Temperature: Given as \( 200^\circ \text{C} \)
- Pressure: Given as \( 1000 \text{ atmospheres} \)
These specific conditions are very high pressure and moderately high temperature, which are typically favorable for the Haber process to maximize \( NH_3 \) production.
### Conclusion
- The reaction is exothermic.
- The yield of \( NH_3 \) is high, approximately \( 98\% \), under the conditions of \( 200^\circ \text{C} \) temperature and \( 1000 \text{ atm} \) pressure.
Putting it all together, the reaction described by the Haber Process is an exothermic reaction that produces [tex]\( NH_3 \)[/tex] with a high yield of approximately [tex]\( 98\% \)[/tex] when conducted at [tex]\( 200^\circ \text{C} \)[/tex] and [tex]\( 1000 \)[/tex] atmospheres of pressure.
