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insens350 [35]
4 years ago
12

The entropy of a system at 337 K increases by 221.7 J/mol•K. The free energy value is found to be –717.5 kJ/mol. Calculate the c

hange in enthalpy of this system. Enter your answer in kJ/mol rounded to the nearest tenths place.
Chemistry
1 answer:
OlgaM077 [116]4 years ago
4 0

<u>Answer:</u> The change in enthalpy for the given system is -642.8 kJ/mol

<u>Explanation:</u>

To calculate the change in enthalpy for given Gibbs free energy, we use the equation:

\Delta G=\Delta H-T\Delta S

where,

\Delta G = Gibbs free energy = -717.5 kJ/mol = -717500 J/mol    (Conversion factor: 1 kJ = 1000 J)

\Delta H = change in enthalpy = ?

T = temperature = 337 K

\Delta S = change in entropy = 221.7 J/mol.K

Putting values in above equation, we get:

-717500J/mol=\Delta H-(337K\times 221.7J/mol.K)\\\\\Delta H=-642787J/mol=-642.8kJ/mol

Hence, the change in enthalpy for the given system is -642.8 kJ/mol

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