Which are spontaneous at high temperatures?Choose one or more:A2H,S(g) + 30,(8) –→ 2H,0(g) + SO,(g)- - 1037 kJ, AS°ºn - - 152.4 J/KAH°rxnR 250,(g) +O,(g) → 280, (g)AH°- 197.8 kJ, AS°- 187.8 J/KC so,(8) + H,0(1) → H,SO,(1)Pxn- - 132.5 kJ, ASº.ΔΗ- 169.9 J/KDS(g) +O2(8) → SO,(8)- 574.0 kJ, AS°nAH°rxn- 124.6 J/KE-none of the above Which are spontaneous at low temperatures?Choose one or more:A° 2H,S(g) + 30,(8) → 2H,0(g) + SO,(g)- 1037 kJ, AS° - - 152.4 J/KAH°.B 2s0,(g) +O,(8) → 2S0,(g)AH°n - - 197.8 kJ, AS°-- - 187.8 J/KrxnrxnCso, (g) + H,O(1) – H,SO,(!)AH°n = - 132.5 kJ, ASºn- 169.9 J/KrxnDO s(g) +02(8) –→ SO,(g)AH° - - 574.0 kJ, AS°,>- 124.6 J/Krxnrxnnone of the above

Answered: Image /qna-images/answer/7985df8a-f4e4-42aa-81f5-0147763e2391.jpg

Which are spontaneous at high temperatures? Choose one or more: A 2H,S(g) + 30,(g) –→ 2H,0(g) + SO,(g) - - 1037 kJ, AS°n - - 152.4 J/K AH° rxn B 250,(g) +O2(g) → 280, (g) AH° - 197.8 kJ, AS° - 187.8 J/K C so,(8) + H,0(1) → H,SO,(1) Pxn - 132.5 kJ, ASº. AH° - 169.9 J/K D S(g) +O2(8) → SO,(8) - 574.0 kJ, AS°n AH°. rxn - 124.6 J/K E none of the above

Which are spontaneous at high temperatures? Choose one or more: A 2H,S(g) + 30,(g) –→ 2H,0(g) + SO,(g) - - 1037 kJ, AS°n - - 152.4 J/K AH° rxn B 250,(g) +O2(g) → 280, (g) AH° - 197.8 kJ, AS° - 187.8 J/K C so,(8) + H,0(1) → H,SO,(1) Pxn - 132.5 kJ, ASº. AH° - 169.9 J/K D S(g) +O2(8) → SO,(8) - 574.0 kJ, AS°n AH°. rxn - 124.6 J/K E none of the above

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 73E: Given the following data 2O3(g) 3O2(g)H = 427 kJ O2(g) 2O(g)H = 495 kJ NO(g) + O3(g) NO2(g) +...

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For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
How is the sign of q, heat, defined? How does it relate to the total energy of the system?
Enthalpy changes often help predict whether or not a process will be spontaneous. What type of reaction is more likely to be spontaneous: an exothermic or an endothermic one? Provide two examples that support your assertion and one counterexample.
Thermodynamics provides a way to interpret everyday occurrences. If you live in northern climates, one common experience is that during early winter, snow falls but then melts when it hits the ground. Both the formation and the melting happen spontaneously. How can thermodynamics explain both of these seemingly opposed events?
Coal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.
Athletic trainers use instant ice packs that can be cooled quickly on demand. Squeezing the pact breaks an inner container, allowing two components to mix and react. This reaction makes the pack become cold. Describe the heat flow for this spontaneous process.
When 1.000 g of gaseous butane, C4H10, is burned at 25C and 1.00 atm pressure, H2O(l) and CO2(g) are formed with the evolution of 49.50 kJ of heat. a Calculate the molar enthalpy of formation of butane. (Use enthalpy of formation data for H2O and CO2.) b Gf of butane is 17.2 kJ/mol. What is G for the combustion of 1 mol butane? c From a and b, calculate S for the combustion of 1 mol butane.
The combustion of methane can be represented as follows: a. Use the information given above to determine the value of H for the combustion of methane to form CO2(g) and 2H2O(l). b. What is Hf for an element in its standard state? Why is this? Use the figure above to support your answer. c. How does H for the reaction CO2(g) + 2H2O (1) CH4(g) + O2(g) compare to that of the combustion of methane? Why is this?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
The formation of aluminum oxide from its elements is highly exothermic. If 2.70 g Al metal is burned in pure O2 to give A12O3, calculate how much thermal energy is evolved in the process (at constant pressure).
At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ/mol and 49 kJ/mol, respectively. a. Calculate H for C6H6(l)3C2H2(g) b. Both acetylene (C2H2) and benzene (C6H6) can be used as fuels. Which compound would liberate more energy per gram when combusted in air?

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