Part 1. Consider the following reaction at 298 K: 2H2(g)+O2(g)---->2H2O(g) ΔH=-483.6 kj/mol Calculate the following quantities:...

Part 1. Consider the following reaction at 298 K: 2H2(g)+O2(g)---->2H2O(g)

ΔH=-483.6 kj/mol

Calculate the following quantities:

ΔSsys=____J(molxK)

ΔSsurr=____J(molxK)

ΔSuniv=____J (molxK)

Part 2. For a particular reaction, ΔH = 168.1 kJ/mol and ΔS = -55.8 J/(mol·K). Calculate ΔG for this reaction at 298 K. Is this system spontaneaus as written, Is it in the reverse direction, Or is it at equilibrium?

Solutions

Expert Solution

Ans 1. The calculation of the answer is given in the picture.

Entropy of the system(∆Ssys)= -1622.8J/mol.k

Entropy of surrounding(∆Ssurr)= +1622.8 J/mol.k

Entropy of universe(∆Suniverse)= 0

Ans2. ∆G = +184728.4 J/mol = 184.728 KJ/mol

(1KJ=1000J)

This System is nonspontaneous.

Yes,it is in the reverse direction , it is not at equilibrium.

The complete calculation of the answer is given in the picture.

queen_honey_blossom answered 1 year ago

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