Consider the following equilibrium reaction and its value of AH°. N204 (g) 4 2 NO2 (g) AH° = 57 kJ Predict whether the reaction will shift towards the products or reactants with a temperature increase. Select one: a. Shift towards the reactants. b. Shift towards the products. O c. The temperature change would have no effect.

Consider the following equilibrium reaction and its value of AH°. N204 (g) 4 2 NO2 (g) AH° = 57 kJ Predict whether the reaction will shift towards the products or reactants with a temperature increase. Select one: a. Shift towards the reactants. b. Shift towards the products. O c. The temperature change would have no effect.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 67E: Consider the reaction 2NO2(g)N2O4(g) For each of the following mixtures of reactants and products at...

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Consider the reaction CO(g)+H2O(g)CO2(g)+H2(g) Use the appropriate tables to calculate (a) G at 552C (b) K at 552C
Hydrogenation, the addition of hydrogen to an organic compound, is an industrially important reaction. Calculate rH, rS, and rG for the hydrogenation of octene, C8H16, to give octane, C8H19 at 25 C. Is the reaction product- or reactant-favored at equilibrium? C8H16(g) + H2(g) C8H18(g) Along with data in Appendix L, the following information is needed for this calculation.
Consider the reaction 2NO2(g)N2O4(g) For each of the following mixtures of reactants and products at 25C, predict the direction in which the reaction will shift to reach equilibrium. a. PNO2=PN2O4=1.0atm b. PNO2=0.21atm,PN2O4=0.50atm c. PNO2=0.29atm,PN2O4=1.6atm
Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
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?
Some metal oxides can be decomposed to the metal and oxygen under reasonable conditions. Is the decomposition of silver(I) oxide product-favored at equilibrium at 25 C? 2 Ag2O(s) 4 Ag(s) + O2(g) If not, can it become so if the temperature is raised? At what temperature does the reaction become product-favored at equilibrium?
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
Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal moles of H2(g) at 1.00 atm and Br2(g) at 1.00 atm were mixed in a 1.00-L flask at 25C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique, and 1.10 1013 molecules were found. For this reaction, calculate the values of K, G, and S.
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?
Calculate K for the formation of methyl alcohol at 100C: CO(g)+2H2(g)CH3OH(g) given that at equilibrium, the partial pressures of the gases are PCO=0.814 atm, PH2=0.274 atm, and PCH3OH=0.0512 atm.
A piece of gold (10.0 g, CAu = 0.129 J/g K) is heated to 100.0 C. A piece of copper (also 10.0 g, CCu = 0.385 J/g K) is chilled in an ice bath to 0 C. Both pieces of metal are placed in a beaker containing 150. g H2O at 20 C. Will the temperature of the water be greater than or less than 20 C when thermal equilibrium is reached? Calculate the final temperature.

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