What is the value for AG at 100 K if AH = 27 kJ/mol and AS = 0.09 kJ/mol.K)?
O A. AG = 2700 kJ/mol
B. AG = -36 kJ/mol
C. AG = 0 kJ/mol
D. AG = 18 kJ/mol

What Is The Value For AG At 100 K If AH = 27 KJ/mol And AS = 0.09 KJ/mol.K)?O A. AG = 2700 KJ/molB. AG

Answers

Answer 1

The value for ΔG = 18 kJ/mol

Further explanation

Given

ΔH = 27 kJ/mol and ΔS = 0.09 kJ/mol.K

T = 100 K

Required

the value for ΔG

Solution

The spontaneous process of a reaction is based on 2 factors :

enthalpy change ΔH decreases and entropy change ΔS increases

ΔG=ΔH-T.ΔS

[tex]\tt \Delta G=27~kJ/mol-100\times 0.09~kJ/mol.K\\\\\Delta G=18~kJ/mol[/tex]


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What is the value for AG at 100 Kif AH = 27 kJ/mol and AS = 0.09 kJ/(mol-K)?
A. AG = 2700 kJ/mol
B. AG = -36 kJ/mol
C. AG = 0 kJ/mol
D. AG = 18 kJ/mol

Answers

Answer:

ΔG =   18KJ/mol

Explanation:

Given data:

ΔS = 0.09 Kj/mol.K

ΔH = 27 KJ/mol

Temperature  = 100 K

ΔG = ?

Solution:

Formula:

ΔG = ΔH - TΔS

ΔS = entropy

ΔH = enthalpy

by putting values,

ΔG =  27 KJ/mol - 100K(0.09 Kj/mol.K)

ΔG =  27 KJ/mol - 9 KJ/mol

ΔG =   18KJ/mol

Answer:

ΔG = 18kJ/mol

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