Question
Asked Jul 31, 2019
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For the reaction

CH4(g) + 2O2(g)CO2(g) + 2H2O(g)

H° = -802.3 kJ and S° = -5.2 J/K

The maximum amount of work that could be done when 1.89 moles of CH4(g) react at 259 K, 1 atm is ________ kJ.

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Expert Answer

Step 1

Given : Change in enthalpy is -802.3 kJ, change in entropy is -5.2 J/K, temperature is 259 K and pressure is 1 atm.

Step 2

Gibbs free energy is defined as the maximum amount of work done by a system at a constant temperature and pressure.

Therefore, it means that Gibb\\'s free energy will always be equal to the total amount of work done.

Gibb\\'s free energy is related to change in enthaly and change in entropy as follows.

AG ΔΗ- TAS
AG= Gibb's free energy
where
AH change in enthalpy
AS= change in entropy
T temperature
help_outline

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AG ΔΗ- TAS AG= Gibb's free energy where AH change in enthalpy AS= change in entropy T temperature

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Step 3

Now, we put the given values in ...

AG -ΔΗ-TΔS
=-802300J 259K x-5.2J/K
=- 802300 J+1346.8 J
= - 800953.2 J
help_outline

Image Transcriptionclose

AG -ΔΗ-TΔS =-802300J 259K x-5.2J/K =- 802300 J+1346.8 J = - 800953.2 J

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