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The following equilibrium is set up in a sealed reaction vessel - HSC - SSCE Chemistry - Question 10 - 2013 - Paper 1
Question 10
The following equilibrium is set up in a sealed reaction vessel. N2O4(g) ⇌ 2NO2(g) ΔH = +54.8 kJ mol⁻¹ Which of the following would INCREASE the yield of nitrog... show full transcript
Worked Solution & Example Answer:The following equilibrium is set up in a sealed reaction vessel - HSC - SSCE Chemistry - Question 10 - 2013 - Paper 1
Step 1
Which of the following would INCREASE the yield of nitrogen dioxide?
Answer
To increase the yield of nitrogen dioxide (NO₂), we must consider changes to the equilibrium as described by Le Chatelier's principle.
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Increase Temperature: Since the reaction is endothermic (ΔH is positive), increasing the temperature will favor the forward reaction to produce more NO₂.
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Increase Pressure: The reaction involves a decrease in the number of moles of gas (2 moles of NO₂ are produced from 1 mole of N₂O₄). Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, thus increasing the yield of NO₂.
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Remove NO₂: By removing some NO₂ from the reaction vessel, the equilibrium will shift to the right to produce more NO₂.
In summary, the effective actions to increase the yield of nitrogen dioxide include raising the temperature, increasing pressure, or removing NO₂ from the system.