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NSWChemistryModule 5: Equilibrium and Acid Reactions

Quick questions on Entropy, enthalpy and Gibbs free energy explained: HSC Chemistry Module 5

4short 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 gibbs free energy?
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Josiah Willard Gibbs combined enthalpy, entropy and temperature into a single quantity that correctly predicts spontaneity:
What is q1?
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State the equation for Gibbs free energy and explain what each of ΔG<0\Delta G < 0, ΔG>0\Delta G > 0 and ΔG=0\Delta G = 0 means for spontaneity. [3 marks]
What is q2?
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A reaction has ΔH=−58 kJ mol−1\Delta H = -58\ \text{kJ mol}^{-1} and ΔS=−176 J K−1mol−1\Delta S = -176\ \text{J K}^{-1}\text{mol}^{-1}. Calculate delta-G at 400 K and state whether the reaction is spontaneous at this temperature. [3 marks]
What is q3?
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Explain why a reaction that is spontaneous (delta-G negative) does not necessarily go to completion. [3 marks]

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