Question

63 points For a particular process, if the change in enthalpy is \( 177.8 \mathrm{~kJ} / \mathrm{mol} \) and the change in entropy is \( 160.5 \mathrm{~J} / \mathrm{molK} \) at \( 25.00^{\circ} \mathrm{C} \), what is the change in free energy, in kilojoules per mole? Your answer should be rounded to the nearest tenth. Include a positive or negative sign with your answer. The change in free energy for this process is 129.9 \( \mathrm{kJ} / \mathrm{mol} \).

          63 points
For a particular process, if the change in enthalpy is \( 177.8 \mathrm{~kJ} / \mathrm{mol} \) and the change in entropy is \( 160.5 \mathrm{~J} / \mathrm{molK} \) at \( 25.00^{\circ} \mathrm{C} \), what is the change in free energy, in kilojoules per mole?
Your answer should be rounded to the nearest tenth. Include a positive or negative sign with your answer.
The change in free energy for this process is 129.9 \( \mathrm{kJ} / \mathrm{mol} \).

63 points
For a particular process, if the change in enthalpy is 177.8 kJ / mol and the change in entropy is 160.5 J / molK at 25.00^∘C, what is the change in free energy, in kilojoules per mole?
Your answer should be rounded to the nearest tenth. Include a positive or negative sign with your answer.
The change in free energy for this process is 129.9 kJ / mol.

Added by Precious C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Anand Jangid

Step 1

We are given the change in enthalpy (\(\Delta H\)) as \(177.8 \, \mathrm{kJ/mol}\), the change in entropy (\(\Delta S\)) as \(160.5 \, \mathrm{J/mol \cdot K}\), and the temperature (\(T\)) at which these changes occur as \(25.00^\circ \mathrm{C}\). Show more…

Show all steps