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Chapter 53: Problem 10

For a chemical reaction with \(K<1\), is \(\Delta G^{\circ}\) positive or negative?

Short Answer

Expert verified
For a chemical reaction with \(K<1\), \(\Delta G^{\circ}\) is positive.

Step by step solution

01

Understanding the relationship

Firstly, understand the relationship between \(\Delta G^{\circ}\) and \(K\). The Gibbs free energy change \(\Delta G^{\circ}\) and the equilibrium constant \(K\) are related by the formula \(\Delta G^{\circ} = -RT \ln K\), where \(R\) is the universal gas constant and \(T\) is the temperature in Kelvin.
02

Sign of \(\Delta G^{\circ}\) when \(K

For \(K<1\), \(\ln K\) (natural log of \(K\)) will be negative since the natural log of any number less than 1 is negative. As a result, \(\Delta G^{\circ}\), which equals \(-RT \ln K\), will be positive, as the product of two negative values resulting in a positive value.

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Most popular questions from this chapter

Eor a chemical reaction with \(K>1\), is \(\Delta G^{\circ}\) positive or negative?

a) What values of \(\Delta H^{\circ}\) indicate that a reaction is energetically favorable? b) What values of \(\Delta S^{\circ}\) indicate that a reaction is entropically favorable?

If \(\Delta H^{\circ}=T \Delta S^{\circ}\), what is the value of \(\Delta G^{\circ}\) ? Predict the value of \(K\) in this case.
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