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NSWChemistryQuick questions

Module 5: Equilibrium and Acid Reactions

Quick questions on Le Chatelier's principle explained: HSC Chemistry Module 5

6short Q&A pairs drawn directly from our worked dot-point answer. For full context and worked exam questions, read the parent dot-point page.

What is pressure changes (gas reactions)?
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Increasing pressure (by decreasing volume) shifts the equilibrium toward the side with fewer moles of gas.
What are temperature changes?
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This is the only disturbance that changes Kc.
What are catalysts?
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A catalyst increases the rate of both forward and reverse reactions equally. It does not shift the equilibrium position and does not change Kc. It only reduces the time taken to reach equilibrium.
What is q1?
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State Le Chatelier's principle and explain why adding a catalyst does not change the position of equilibrium. [3 marks]
What is q2?
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For the reaction N2O4(g)⇌2NO2(g)N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}, ΔH=+57 kJ mol−1\Delta H = +57 \text{ kJ mol}^{-1}, predict and justify the shift in equilibrium position when (a) the temperature is increased, (b) the volume is halved. [2+2 marks]
What is q3?
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Consider 2SO2(g)+O2(g)⇌2SO3(g)2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}, ΔH=−198 kJ mol−1\Delta H = -198 \text{ kJ mol}^{-1}. (a) State the effect on yield of SO3SO_3 of increasing temperature. (b) State the effect of increasing pressure.

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