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13 Dec 2019

For a given reaction, ΔH = -24.2 kJ/mol and ΔS = -55.5 J/K-mol. The reaction will have ΔG = 0 at ???? K. Assume that ΔH and ΔS do not vary with temperature.

The value of ΔS° for the oxidation of solid elemental sulfur to gaseous sulfur trioxide,

2S (s, rhombic) + 3O2(g) → 2SO3 (g)

is ??? J/K ∙ mol.



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Trinidad Tremblay
Trinidad TremblayLv2
17 Dec 2019

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Related questions

For a given reaction, ΔH= -24.2 kJ/mol and ΔS=-77.0 kJ/mol. The reaction will have ΔG= 0 at _____ K. Assume ΔH and ΔS do not vary with temperature.

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Given the following information determine the reaction Gibbs energy for the formation of hydrazine (N2H4) at 298 K 2NH3(g)→ N2H4(l)+H2(g) ΔfH°(NH3(g))=-46.11 kJ mol-1, S°(NH3(g))=192.45 J mol-1 K-1 ΔfH°(N2H4(l))=50.63 kJ mol-1, S°(N2H4(s))=121.21 J mol-1 K-1 ΔfH°(H2(g))=0 kJ mol-1, S°(H2(g))=130.7 J mol-1 K-1 Answer to TWO decimals places in kJ mol-1

A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.)

2 SO3(g) → 2 SO2(g) + O2(g)
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ΔH° = kJ

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Reaction is spontaneous _________above this temperaturebelow this temperatureat all temperaturesat no temperature.

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