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Q: consider the following thermodynamic data:


ΔHf {NO,g} = +90.4kJ/mol S {NO} = 210.6 J/mol*K

S {O2 , g} = 205.0 J/mol*K S {N2, g} = 191.5 J/mol *K

a) calculate ΔG for this reaction at 100.0 Celsius:

N2(g) + O2 (g)-----> 2NO (g)

b) Assuming standard conditions, at what temperature (s) wouldthe reaction above be reversible?

thank you in advance.

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Related questions


Show transcribed image text
Use data from the table below to calculate the equilibrium constants at 25?C for each reaction.

Standard Thermodynamic Quantities for Selected Substances
at 25?C

Substance ?H?f(kJ/mol) ?G?f(kJ/mol) S?(J/mol?K)
H2(g) 0 0 130.7
N2(g) 0 0 191.6
O2(g) 0 0 205.2
NO(g) 91.3 87.6 210.8
CO(g) -110.5 -137.2 197.7
CO2(g) -393.5 -394.4 213.8
H2S(g) -20.6 -33.4 205.8
S2(g) 128.6 79.7 228.2

Part A

2CO(g)+O2(g)?2CO2(g)

Express your answer using two significant figures.
K =

SubmitPrevious AnswersRequest Answer

Part B

N2(g)+O2(g)?2NO(g)

Express your answer using two significant figures.
K =

Submit

The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury (II) oxide.
HgO(s) --> Hg(l) + 1/2O2(g) ΔH° = 90.84 kJ


Use the data given below to determine DS = and the temperature, at which this reaction will become spontaneous under standard conditions.
S°(Hg) = 76.02 J/K· mol
S°(O2) = 205.0 J/K· mol
S°(HgO) = 70.29 J/K· mol

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