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owLV2 | Online teachin X + sjc.cengagenow.com/ilrn/takeAssignme ty.do?locator-assignment nmentSessionLocator- assignment-take Chapter 10: Mastery 1 pts 1 pts f pts 2req 1 pts 2req 1. Compare Absolute Entropies Use the References to access important values if needed for this question 2. Predict the Sign of S Consider the reaction: 2HBr(g) :H2 (g)" Br(1) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.72 moles of HBr(g) react at standard 4. Standard Entropy of Reaction Question J/K Question f pts 2req Submit Answer Retry Entire Group 9 more group attempts remaining 6. AG: Predict Signs 7. AG: Enthalpy, Entropy and Temper... pts 8. AG: Calculate Temperature Limit 1 pts 2req 1 pts 2req s of Refining Met... 1 pts 2req 10. AG from Free Energies of Form pts 2req

Explanation / Answer

we have:

Sof(HBr(g)) = 198.695 J/mol.K

Sof(H2(g)) = 130.684 J/mol.K

Sof(Br2(l)) = 152.2 J/mol.K

we have the Balanced chemical equation as:

2 HBr(g) ---> H2(g) + Br2(l)

deltaSo rxn = 1*Sof(H2(g)) + 1*Sof(Br2(l)) - 2*Sof( HBr(g))

deltaSo rxn = 1*(130.684) + 1*(152.2) - 2*(198.695)

deltaSo rxn = -114.506 J/K

As per reaction, this is when 2 mol of HBr reacts

So,

for 1.72 moles of N2,

deltaSo rxn = 1.72 moles *-114.506 J/K / 2 mol

= - 98.5 J/K

Answer: - 98.5 J/K

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