Consider the following endothermic reaction taking place in a closed vessel - HSC - SSCE Chemistry - Question 14 - 2016 - Paper 1
Question 14
Consider the following endothermic reaction taking place in a closed vessel.
$$N_2O_4(g) \rightleftharpoons 2NO_2(g)$$
Which of the following actions would cause m... show full transcript
Worked Solution & Example Answer:Consider the following endothermic reaction taking place in a closed vessel - HSC - SSCE Chemistry - Question 14 - 2016 - Paper 1
Step 1
Adding a catalyst
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Answer
Adding a catalyst does not affect the position of equilibrium; it only speeds up the rate at which equilibrium is reached. Therefore, this action will not increase the production of N2O4.
Step 2
Decreasing the volume
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Answer
Decreasing the volume of a gaseous reaction shifts the equilibrium towards the side with fewer moles of gas. In this reaction, the left side (N2O4) has 1 mole, while the right side has 2 moles. Therefore, decreasing the volume will favor the formation of N2O4, resulting in more being produced.
Step 3
Decreasing the pressure
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Answer
Decreasing the pressure in a system shifts the equilibrium towards the side with more moles of gas. Hence, it will favor the formation of NO2, resulting in less N2O4 being produced.
Step 4
Increasing the temperature
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Answer
Since the reaction is endothermic, increasing the temperature will shift the equilibrium to favor the formation of the products, which is NO2, rather than N2O4. Thus, this action will not result in more N2O4 being produced.
