The oxidation of glucose to carbon dioxide and water is represented by the following reaction, whether the oxidation occurs by combustion in the laboratory or by biological oxidation in living cells: C6H12O6+6O2⇌6CO2+6H2O When combustion is carried out under controlled conditions in the laboratory, the reaction is highly exothermic, with an enthalpy change (ΔH) of −673kcal/mol. As you know, ΔG for this reaction at 25∘C is −686kcal/mol, so the reaction is also highly exergonic. Part A Explain what the ΔH and ΔG values mean. What do the negative signs mean in each case? Drag the terms on the left to the appropriate blanks on the right to complete the sentences. Terms can be used once, more than once, or not at all.

∆H is known as the change in enthalpy. When the change in enthalpy is negative, it simply means that heat is given out during the reaction. Therefore, we refer to the reaction as an exothermic reaction.

Similarly, ∆G is known as change in free energy. When the change in free energy is negative, it implies that the reaction is spontaneous as written. This is called an exergonic reaction.

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