The synthesis of ammonia gas from nitrogen gas and hydrogen gasrepresent a class

Question

The synthesis of ammonia gas from nitrogen gas and hydrogen gasrepresent a classic case in which a knowledge of kinetics andequilibrium was used to make a desired chemical reactioneconomically feasible. Explain how each of the following conditions helps to maximazethe yeild of ammonia. a. running the reation at an elevated temperarure b. removing the ammonia from the reaction mixture as itforms c. using a catalyst d. running the reaction at high pressure
Explain how each of the following conditions helps to maximazethe yeild of ammonia. a. running the reation at an elevated temperarure b. removing the ammonia from the reaction mixture as itforms c. using a catalyst d. running the reaction at high pressure

Explanation / Answer

           N2 + 3 H2 ----------> 2 NH3 a) Nitrogen is a relatively unreactive species. So it does notreact at low temperatures. Only at an elevated temperature, does itcombine with hydrogen to form ammonia. Hence higher temperaturehelps to increase the yield of ammonia. b) When ammonia is removed from the mixture as it forms, itsconcentration in the equilibrium mixture decreases. So the equilibrium of the reaction is driven to the right andmore ammonia is formed. c) A catalyst such as iron oxide is usually used in the process.The presence of the catalyst increases the rate of the reaction. Itdoes not participate in the reaction but supplies the necessaryactivation energy for the reactents to react. d) From the equation, we can see that 4 moles of reactant reactto form 2 moles of product. As there is a decrease in the number ofmoles, a increase in pressure will favour the forward reaction. somore ammonia will be formed at higher pressure. a) Nitrogen is a relatively unreactive species. So it does notreact at low temperatures. Only at an elevated temperature, does itcombine with hydrogen to form ammonia. Hence higher temperaturehelps to increase the yield of ammonia. b) When ammonia is removed from the mixture as it forms, itsconcentration in the equilibrium mixture decreases. So the equilibrium of the reaction is driven to the right andmore ammonia is formed. c) A catalyst such as iron oxide is usually used in the process.The presence of the catalyst increases the rate of the reaction. Itdoes not participate in the reaction but supplies the necessaryactivation energy for the reactents to react. d) From the equation, we can see that 4 moles of reactant reactto form 2 moles of product. As there is a decrease in the number ofmoles, a increase in pressure will favour the forward reaction. somore ammonia will be formed at higher pressure.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.