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For the reaction nh4cl (s) → nh3 (g) + hcl (g) at 25°c, 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?

Respuesta :

kenmyna
   The  of the reaction is  91.07  Kj    and the  reaction  is  will  be    Spontaneous   in the  forward direction

      Explanation
  by  use of  ΔG =ΔH- TΔs   formula  calculate for ΔG
ΔG =?
ΔH= 176  kj/mol
Δs= 0.285 kj/mol.k
T= 25 + 273 = 298 K

ΔG  is therefore = 176 - 298 (0.285)= 91.07 Kj

since ΔG  is positive the  reaction   will not  be  spontaneous   in the forward direction

The value of ΔG for the given reaction is 91.07 kJ, and reaction is not spontaneous as it absorbs the energy.

How we calculate the Gibb's free energy of reaction?

Gibb's free energy of any reaction can be calculated as:

ΔG = ΔH - TΔS, where

ΔH = change in enthalpy of the reaction = 176 kJ/mole

ΔS = change in entropy of the reaction = 0.285 kJ/mol.K

T = temperature of the reaction = 25°C = 298K

Now we calculate the free energy change for the reaction given below by putting all these values in the free energy change equation.

NH₄Cl(s) → NH₃(g) + HCl(g)

ΔG = 176 - (298 × 0.285) = 91.07 kJ

Hence, reaction is not spontaneous because we get a positive value of free energy of the reaction i.e. 91.07 kJ.

To know more about Gibb's free energy change, visit the below link:

https://brainly.com/question/9908454

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