Question:
Calculate the free energy change for a certain reaction at \(300\) K if \(\Delta H\) is \(60\) kJ and \(\Delta S\) is \(-120\text{JK}^{-1}\).
Calculate the free energy change for a certain reaction at \(300\) K if \(\Delta H\) is \(60\) kJ and \(\Delta S\) is \(-120\text{JK}^{-1}\).
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Use delta G = delta H - T delta S, keeping the entropy in kJ per kelvin.
Updated On: Nov 12, 2026
- \(24.0\) kJ
- \(-35.5\) kJ
- \(96.0\) kJ
- \(-57.5\) kJ
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The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept
The free energy change is \(\Delta G=\Delta H-T\Delta S\).
Step 2: Unit conversion
\(\Delta S=-120\text{ J K}^{-1}=-0.120\text{ kJ K}^{-1}\).
Step 3: Calculation
\(\Delta G=60-300\times(-0.120)=60+36=96\) kJ.
Step 4: Compare the options
This is option (C).
Final Answer:
The free energy change is +96.0 kJ. \[ \boxed{\text{(C) }96.0\text{ kJ}} \]
The free energy change is \(\Delta G=\Delta H-T\Delta S\).
Step 2: Unit conversion
\(\Delta S=-120\text{ J K}^{-1}=-0.120\text{ kJ K}^{-1}\).
Step 3: Calculation
\(\Delta G=60-300\times(-0.120)=60+36=96\) kJ.
Step 4: Compare the options
This is option (C).
Final Answer:
The free energy change is +96.0 kJ. \[ \boxed{\text{(C) }96.0\text{ kJ}} \]
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