e COg H2Og02g H2g 4 Commercially ammonia NH3 is produced f

e.) CO(g) + H2O(g)02(g) + H2(g) 4. Commercially, ammonia (NH3) is produced from nitrogen (N2) and hydrogen (H2) using the Haber process: N2(g) + 3H2(g) 2NH3(g) This reaction is exothermic. Which of the following would INCREASE the amount of NH3 obtained (i.e., maximize the yield of NH3) at equilibrium? i. Decrease the pressure. ii. Increase the temperature. 111. . iv. Increase the concentration of NH3. V. Increase the concentration of N2 Decrease the concentration of H2. a. b. C. i, ii, iv and v i and iii ii and iii d.i only e. i, iv and v

Solution

The correct answer is (D). To get the maximum amount of NH₃, the forward reaction should be favored. It could be achieved by increasing the concentration of N₂ as the forward reaction uses N₂ to convert to NH₃. Due to increase in concentration, the forward reaction will speed up temporarily and more NH₃ is produced.