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Chapter 17: Problem 33

What is a coupled reaction? What is its importance in biological reactions?

Short Answer

Expert verified
A coupled reaction is a chemical reaction where an energy-releasing (exergonic) reaction happens alongside an energy-absorbing (endergonic) reaction. The energy released by the exergonic reaction drives the endergonic reaction. In biological systems, coupled reactions are crucial, allowing energetically unfavorable reactions, necessary for life processes, to take place by utilizing the energy produced from energetically favorable reactions.

Step by step solution

01

Understand and Define Coupled Reaction

A coupled reaction is a type of chemical reaction where an energetically unfavorable reaction occurs simultaneously with an energetically favorable one. The favorable reaction provides the energy necessary for the unfavorable one to occur, and hence the two reactions are 'coupled'.
02

Importance in Biological Reactions

The importance of coupled reactions in biological context lies in the energy transfer. In a living organism, many processes require energy, that is often derived from unfavorable reactions. These reactions can't proceed without an external energy source. This is where coupled reactions come into play. The energy released from favorable reactions, structurely or spatially related, can be used to drive the unfavorable reactions, enabling biological processes to take place.

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Most popular questions from this chapter

The sublimation of carbon dioxide at \(-78^{\circ} \mathrm{C}\) is $$ \mathrm{CO}_{2}(s) \longrightarrow \mathrm{CO}_{2}(g) \quad \Delta H_{\mathrm{sub}}=62.4 \mathrm{~kJ} / \mathrm{mol} $$ Calculate \(\Delta S_{\text {sub }}\) when \(84.8 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) sublimes at this temperature.

For a reaction with a negative \(\Delta G^{\circ}\) value, which of the following statements is false? (a) The equilibrium constant \(K\) is greater than one. (b) The reaction is spontaneous when all the reactants and products are in their standard states. (c) The reaction is always exothermic.

Describe two ways that you could measure \(\Delta G^{\circ}\) of a reaction.

The standard enthalpy of formation and the standard entropy of gaseous benzene are \(82.93 \mathrm{~kJ} / \mathrm{mol}\) and \(269.2 \mathrm{~J} / \mathrm{K} \cdot \mathrm{mol},\) respectively. Calculate \(\Delta H^{\circ}, \Delta S^{\circ}\) and \(\Delta G^{\circ}\) for the process at \(25^{\circ} \mathrm{C}\). $$ \mathrm{C}_{6} \mathrm{H}_{6}(l) \longrightarrow \mathrm{C}_{6} \mathrm{H}_{6}(g) $$ Comment on your answers.

Under what conditions does a substance have a standard entropy of zero? Can a substance ever have a negative standard entropy?
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