Consider the reactionN₂(g) + 3H₂(g)2NH3(g)Using the standard thermodynamic data in the tables linked above, calculate AGrxn for this reaction at 298.15K if thepressure of each gas is 14.60 mm Hg.ANSWER:Submit AnswerUse the References to access important values if needed for this question.AkJ/molRetry Entire Group 9 more group attempts remainingW-Next>Save and Exit

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Consider the reaction N₂(g) + 3H₂(g)2NH3(g) Using the standard thermodynamic data in the tables linked above, calculate AGrxn for this reaction at 298.15K if the pressure of each gas is 14.60 mm Hg. kJ/mol ANSWER: Use the References to access important values if needed for this question. Submit Answer Retry Entire Group 9 more group attempts remaining

Consider the reaction N₂(g) + 3H₂(g)2NH3(g) Using the standard thermodynamic data in the tables linked above, calculate AGrxn for this reaction at 298.15K if the pressure of each gas is 14.60 mm Hg. kJ/mol ANSWER: Use the References to access important values if needed for this question. Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 74QAP: Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to...

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The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is 2H2(g)+O2(g)2H2O(l)K=1.281083 a. Calculate and G at 298 K for the fuel cell reaction. b. Predict the signs of H and S for the fuel cell reaction. c. As temperature increases, does the maximum amount of work obtained from the fuel cell reaction increase, decrease, or remain the same? Explain.
Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?
Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 2.00 with all other ionic species at 0.100 M? (c) Is the reaction spontaneous at a pH of 5.00 with all other ionic species at 0.100 M? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M?
The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing Mn2+ ions. These ions are then oxidized to the deeply colored MnO4 ions by periodate ion (IO4) in acid solution. a. Complete and balance an equation describing each of the above reactions. b. Calculate and G at 25C for each reaction.
When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced equation for the reaction. How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCl? How can you harness this reaction to do useful work?
Hydrazine, N2H4, can be used as the reducing agent in a fuel cell. N2H4(aq) + O2(aq) N2(g) + 2 H2O () (a) If rG for the reaction is 598 kJ, calculate the valueof E expected for the reaction. (b) Suppose the equation is written with all coefficients doubled. Determine rG and E for this new reaction.
Among other things, an ideal fuel for the control thrusters of a space vehicle should decompose in a spontaneous exothermic reaction when exposed to the appropriate catalyst. Evaluate the following substances under standard state conditions as suitable candidates for fuels. (a) Ammonia: 2NH3(g)N2(g)+3H2(g) (b) Diborane: B2H6(g)2B(g)+3H2(g) (c) Hydrazine: N2H4(g)N2(g)+2H2(g) (d) Hydrogen peroxide: H2O2(l)H2O(g)+12O2(g)
In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g)+4H2(g)NH3(g)+3H2O(g)H=637kJ (a) Calculate H when one mole of hydrogen gas reacts. (b) What is H when 10.00 g of NH3(g) are made to react with an excess of steam to form HN3(g) and H2 gases?
9.72 Although it can be a nuisance when a laptop computer freezes up and needs to be rebooted, we accept that as somewhat inevitable. But clearly the need to occasionally reboot the control system for the power grid would not be acceptable. Use the web to research ways that engineers ensure the reliability of crucial systems like the control infrastructure of the grid, and write a paragraph summarizing the main strategies employed.
If you calculate a value for G for a reaction using the values of Gf in Appendix 4 and get a negative number, is it correct to say that the reaction is always spontaneous? Why or why not? Free energy changes also depend on concentration. For gases, how is G related to the pressure of the gas? What are standard pressures for gases and standard concentrations for solutes? How do you calculate G for a reaction at nonstandard conditions? The equation to determine G at nonstandard conditions has Q in it: What is Q? A reaction is spontaneous as long as G is negative; that is, reactions always proceed as long as the products have a lower free energy than the reactants. What is so special about equilibrium? Why dont reactions move away from equilibrium?
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
Calculate E°, G°, and K at 25°C for the reaction 3Mn2+(aq)+2MnO4(aq)+2H2O5MnO2(s)+4H+(aq)