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xxMikexx [17]
3 years ago
11

Part A Find ΔS∘ for the reaction between nitrogen gas and hydrogen gas to form ammonia: 12N2(g)+32H2(g)→NH3(g) Express your answ

er using one decimal place. ΔS∘Δ S ∘ = J/K Previous Answer Request Answer Incorrect; Try Again; 3 attempts remaining Part B Complete previous part(s) Provide Feedback
Chemistry
1 answer:
inessss [21]3 years ago
7 0

Answer:

\Delta S^{0} for the given reaction is -99.4 J/K

Explanation:

Balanced reaction: \frac{1}{2}N_{2}(g)+\frac{3}{2}H_{2}(g)\rightarrow NH_{3}(g)

\Delta S^{0}=[1mol\times S^{0}(NH_{3})_{g}]-[\frac{1}{2}mol\times S^{0}(N_{2})_{g}]-[\frac{3}{2}mol\times S^{0}(H_{2})_{g}]

where S^{0} represents standard entropy.

Plug in all the standard entropy values from available literature in the above equation:

\Delta S^{0}=[1mol\times 192.45\frac{J}{mol.K}]-[\frac{1}{2}mol\times 191.61\frac{J}{mol.K}]-[\frac{3}{2}mol\times 130.684\frac{J}{mol.K}]=-99.4J/K

So, \Delta S^{0} for the given reaction is -99.4 J/K

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