Your (lecture) course textbook uses the Haber synthesis of ammonia, an exothermi

Question

Your (lecture) course textbook uses the Haber synthesis of ammonia, an exothermic reaction to illustrate many concepts of chemical equilibrium, in specific the effects of concentration, pressure volume, and temperature chances on the equilibrium Write a balanced chemical equilibrium reaction foe the synthesis of ammonia by the Haber method. How docs adding nitrogen gas affect the equilibrium? How does adding hydrogen gas affect the equilibrium? How docs adding ammonia gas affect the equilibrium? How docs decreasing the pressure (increasing the volume) affect the equilibrium? How docs cooling the reaction affect the equilibrium? Based on your previous answers, what conditions of temperature and pressure will maximize production for a system engineered to synthesize ammonia by the Haber method?

Explanation / Answer

2) addition of reactants shifts the equilibrium to right.

     So, addition of N2 gas shifts the equilibrium to right.

3) addition of reactants shifts the equilibrium to right.

     So, addition of H2 gas shifts the equilibrium to right.

4) addition of products shifts the equilibrium to left.

     So, addition of NH3 gas shifts the equilibrium to left.

5) no of moles of products - no of moles of reactants = 2-4 = -2

Therefore, decreasing the presssure shifts the equilibrium to left.

6) Given reaction is exothermic.

    All exothermic reactions are favored by decreasing temperature.

   Therefore, cooling the reaction shifts the equilibrium to right.

7) Low temperature and high pressure maximize the production of ammonia.

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