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horrorfan [7]
3 years ago
14

Calculate AS° for the reaction below: N2(g)+202(g) 2NO2(g) where ASo for N2(g), O2(g), & NO2(g), respectively, is 191.5, 205

.0, & 240.5 J/mol-K -156.0 J/K 156.0 J/K 120.5 J/K -120.5 J/K O OOO
Chemistry
1 answer:
nignag [31]3 years ago
5 0

Answer:

ΔS Rx = -120, 5 J/K

Explanation:

The ΔS in a reaction is defined thus:

ΔS Rx = ∑ n S°products - ∑ m S°reactants

For the reaction:

N₂(g) + 2 O₂(g) → 2NO₂(g)

ΔS Rx = 2 mol × 240,5 \frac{J}{mol.K} - [ 1 mol × 191,5 \frac{J}{mol.K} + 2 mol × 205,0 \frac{J}{mol.K}]=

<em>ΔS Rx = -120, 5 J/K</em>

A negative value in ΔS means a negative entropy of the process. Doing this process entropycally unfavorable.

I hope it helps!

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