CIE Nov 2014 v3 Paper 2 Q2

Answers available below

The Haber process for the manufacture of ammonia, NH3, was originally devised at the start of the 20th century and was developed into a full-scale industrial process by Carl Bosch in 1913. PMT The key step in the process is the reversible reaction of nitrogen and hydrogen in the presence of an iron catalyst. N2(g) + 3H2(g) 2NH3(g) H = 92 kJ mol1 (a) The hydrogen for this reaction can be formed by reacting methane with steam, during which carbon monoxide is also produced. Write an equation for this reaction.[1] (b) Use the Boltzmann distribution shown to explain why a catalyst increases the rate of this reaction. number of molecules kinetic energy[4] (c) Draw a three-dimensional diagram to show the shape of an ammonia molecule. Name this shape and state the bond angle. shapebond angle[3]UCLES 2014 9701/23/O/N/14<br /> PMT (d) The Haber process is typically carried out at a temperature of 400 C. (i) With reference to Le Chateliers Principle and reaction kinetics, state and explain one advantage and one disadvantage of using a higher temperature.[4] (ii) State the expression for the equilibrium constant, Kp, for the formation of ammonia from nitrogen and hydrogen in the Haber process. Kp = (iii) 2.00 moles of nitrogen and 3.00 moles of hydrogen were put in a vessel and left to reach equilibrium. At equilibrium, the pressure was 2.00107 ammonia. Pa and the mixture contained 1.60 moles of Calculate Kp. Include the units. [1] Kp =units =[5] [Total: 18]UCLES 2014 9701/23/O/N/14 [Turn over<br />

Show answer