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For the reaction NH4 Cl(s) > NH3(g) + HCl(g) at 664 celsius ΔH= 176 kJ/mol, and ΔS = 0.285 kJ/ (mol K)
What is the ΔG, and will this reaction be spontaneous in the forward direction?

A) -91 kJ/mol; yes
B) 91 kJ/mol; yes
C)91 kJ/mol; no
D) 91 kJ/mol; no

Respuesta :

pstnonsonjoku

From the calculation and the value of the free energy change(-91 kJ/mol), the reaction is spontaneous.

What is the free energy change?

The sign of the free energy change determines whether the reaction will be spontaneous or not. A reaction is spontaneous only when the free energy change is negative.

Using;

ΔG=  ΔH -  TΔS

ΔG= 176 kJ/mol - [937 K *  0.285 kJ/ (mol K)]

ΔG=-91 kJ/mol

Hence, the reaction is spontaneous.

Learn more about free energy:https://brainly.com/question/15319033

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