For higher yields of ammonia increase in temperature is replaced by which of the following?
Correct answer: D. All of these
- A. Increasing pressure
- B. Decreasing volume
- C. Using catalyst
- D. All of these
Explanation
The reaction is shown in the image attached. On the reactant side, there are 4 moles and on the product side, there are 2 moles. On increasing the pressure, the position of equilibrium will shift towards the side that has less moles of gas, i.e. the product side. Therefore, a greater yield of ammonia will be obtained. Hence A is correct. Remember that YIELD depends on the position of equilibrium. Adding a catalyst makes absolutely no difference to the position of equilibrium - it only speeds up the rate at which a reaction reaches dynamic equilibrium.Decreasing the volume would result in increased pressure. Therefore, the correct answer is all of these: increasing pressure, decreasing volume, and using a catalyst can all be used to increase the yield of ammonia.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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