Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
100%

Ammonia is a pungent, colourless gas. Its major use is in fertilisers as salts, such as, ammonium nitrate and ammonium sulphate. The Haber-Bosch process, as shown below, is an important reaction that produces ammonia.

 

(a) At 127 °C the following equilibrium concentrations were found for the Haber-Bosch process.

 

                                         [H2] = 3.1 × 10–3 M                 

                                    [N2] = 8.5 × 10–1 M

                                    [NH3] = 3.1 × 10–2 M

Write the equilibrium constant expression for this reaction.                                                  

(b) Calculate the value of Kc for this reaction and predict the whether the products or reactants will be favoured at equilibrium.                                                                                                     

 

(c) Considering the Haber-Bosch reaction, predict and explain the effect on the equilibrium for the reaction, in response to the following:                                                                               

  • Decreasing temperature
  • Increasing the concentration of nitrogen gas
  • Decreasing pressure
  • Removing the catalyst
  • Reducing the volume of the reaction vessel.

 

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