O KINETICS AND EQUILIBRIUM Using the van't Hoff equation to predict K ata different tempera... At-15.9 °C the concentration equilibrium constant K = 4.1 for a certain reaction. Here are some facts about the reaction: If the reaction is run at constant pressure, 90.0 kJ/mol of heat are absorbed. . If the reaction is run at constant pressure, the volume increases by 10.%. The net change in moles of gases is 2. Yes x10 Using these facts, can you calculate K at 1.9 °C? C No. X If you said yes, then enter your answer at right. Round it to 2 significant digits. Explanation Check O KINETICS AND EQUILIBRIUM Using the van't Hoff equation to predict K at a different tempera... Yes. Using these facts, can you calculate K at 1.9 °C? No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K will be bigger If you said no, can you at least decide whether K at Yes, and K will be с 1.9 °C will be bigger or smaller than K at-15.9 °C? smaller. С No. Explanation Check

O KINETICS AND EQUILIBRIUM Using the van't Hoff equation to predict K ata different tempera... At-15.9 °C the concentration equilibrium constant K = 4.1 for a certain reaction. Here are some facts about the reaction: If the reaction is run at constant pressure, 90.0 kJ/mol of heat are absorbed. . If the reaction is run at constant pressure, the volume increases by 10.%. The net change in moles of gases is 2. Yes x10 Using these facts, can you calculate K at 1.9 °C? C No. X If you said yes, then enter your answer at right. Round it to 2 significant digits. Explanation Check O KINETICS AND EQUILIBRIUM Using the van't Hoff equation to predict K at a different tempera... Yes. Using these facts, can you calculate K at 1.9 °C? No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K will be bigger If you said no, can you at least decide whether K at Yes, and K will be с 1.9 °C will be bigger or smaller than K at-15.9 °C? smaller. С No. Explanation Check

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.108PAE: 12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant...

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Wet limestone is used to scrub SO2 gas from the exhaust gases of power plants. One possible reaction gives hydrated calcium sulfite: CaCO3(s) + SO2(g) + H2O() CaSO3 H2O(s) + CO2(g) Another reaction gives hydrated calcium sulfate: CaCO3(s) + SO2(g) + H2O() + O2(g) CaSO4 H2O(s) + CO2(g) (a) Which reaction is more product-favored at equilibrium? Use the data in the table below and any other information needed in Appendix L to calculate rG for each reaction at 25 C. (b) Calculate rG for the reaction CaSO3 H2O(s) + O2(g) CaSO4 H2O(s) Is this reaction product- or reactant-favored at equilibrium?
12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant into a lake and estimates that this may warm the water locally to 25 °C. One question to be considered is the effect of this temperature change on the uptake of CO2 by the water. The equilibrium constant for the reaction CO2+H2OH2CO3 ; is K=1.7103 at 25 °C. Because bonds form, the reaction is exothermic. (a) Will this reaction progress further toward products at higher temperatures near the water discharge with its warmer water than it would in the cooler lake water? Explain your reasoning. (b) Carbonic acid has a Kaof 2.5104 at 25 °C. What is the equilibrium constant for the CO2+2H2OHCO3+H3O+? (c) What additional factor should the engineer be considering about CO2 gas, probably before considering this reaction chemistry?
The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).
Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
Consider the following reaction at 298 K: 2SO2(g)+O2(g)2SO3(g) An equilibrium mixture contains O2(g) and SO3(g) at partial pressures of 0.50 atm and 2.0 atm, respectively. Using data from Appendix 4, determine the equilibrium partial pressure of SO2 in the mixture. Will this reaction be most favored at a high or a low temperature, assuming standard conditions?
Red phosphorus is formed by heating white phosphorus. Calculate the temperature at which the two forms are at equilibrium, given white P: H f =0.00 kJ/mol; S =41.09 J/mol K red P: H f =17.6 kJ/mol; S =22.80 J/mol K
Follow the directions of Problem 27 for each of the reactions in Question 20.
As O2(l) is cooled at 1 atm, it freezes at 54.5 K to form solid I. At a lower temperature, solid I rearranges to solid II, which has a different crystal structure. Thermal measurements show that H for the I II phase transition is 743.1 J/mol, and S for the same transition is 17.0 J/K mol. At what temperature are solids 1 and II in equilibrium?
Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?
One reaction that occurs in human metabolism is For this reaction G= 14 kJ at 25c. a. Calculate K for this reaction at 25C. b. In a living cell this reaction is coupled with the hydrolysis of ATP. (See Exercise 75.) Calculate G and K at 25C for the following reaction: Glutamicacid(aq)+ATP(aq)+NH3(aq)Glutamine(aq)+ADP(aq)+H2PO4(aq)
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