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1) What is the value of G at 120.0 K for a reaction in which H = +35 kJ/mol and S = 1.50
kJ/(molK)?

Sagot :

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Answer:

ΔG = -145kJ/mol

Explanation:

To solve this question we must use the change in Gibbs free energy:

ΔG = ΔH - TΔS

Where ΔG is change in Gibbs free energy = ?

ΔH is enthalpy change = +35kJ/mol

T is absolute temperature = 120.0K

And ΔS is change in entropy = 1.50kJ/molK

Replacing:

ΔG = 35kJ/mol - 120.0K*1.50kJ/molK

ΔG = 35kJ/mol - 180kJ/mol

ΔG = -145kJ/mol

Value of G at given temperature 120.0 Kelvin for the given reaction is -145 kJ/mol.

Temperature reaction based problem:

Given in the question:

ΔH = +35 kJ/mol

ΔS = 1.50 kJ/mol

Temperature = 120° K

Find the value of ΔG at 120° K

Computation:

  • ΔG = ΔH – TΔS
  • ΔG = 35 - 120(1.5)
  • ΔG = 35 - 180ΔG = -145 kJ/mol

Value of G at 120.0 K temperature for a reaction = -145 kJ/mol

Find more about information about 'temperature'.

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