Chapter 22: Problem 43

The enthalpy change in the denaturation of a certain protein is \(125 \mathrm{~kJ} / \mathrm{mol}\). If the entropy change is \(397 \mathrm{~J} / \mathrm{K} \cdot\) mol, calculate the minimum temperature at which the protein would denature spontaneously.

Short Answer

Expert verified

The minimum temperature at which the protein would denature spontaneously is greater than 315 K

Step by step solution

Understand the Gibbs free energy equation

The Gibbs free energy equation is given by ΔG = ΔH - TΔS. In order for a process to occur spontaneously, ΔG should be negative. For denaturation to take place, it means ΔH - TΔS must be less than zero.

Express the required temperature from the equation

To find the minimum temperature for spontaneous denaturation, rearrange the Gibbs free energy equation to obtain the expression for temperature. From ΔH - TΔS < 0, we get T > ΔH / ΔS.

Substitute the values into the equation

Substituting the given values ΔH = 125 kJ/mol = 125000 J/mol and ΔS = 397 J/K•mol into the equation, we have: T > 125000 / 397

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The enthalpy change in the denaturation of a certain protein is \(125 \mathrm{~kJ} / \mathrm{mol}\). If the entropy change is \(397 \mathrm{~J} / \mathrm{K} \cdot\) mol, calculate the minimum temperature at which the protein would denature spontaneously.

Short Answer

Step by step solution

Understand the Gibbs free energy equation

Express the required temperature from the equation

Substitute the values into the equation

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