What is the correct Kc expression for the reaction below? 2PBO(s) + 02(g) = 2P6O2(s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. [Pbo] (02] K = [PbO2]? a K = = [02] b 1 K = [02] [PbO,]? [Pbo] [0,] d K = = [PbO]*[O2] e The reaction for the decomposition of carbonyl bromide gas is shown below. What is the Kp for this reaction, expressed using standard units? COBr2 (g) = CO(g) + Br2 (g) Kc = 0.190 at 73°C Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 0.190 b 1.15 5.47 d 15.7 e 540.

What is the correct Kc expression for the reaction below? 2PBO(s) + 02(g) = 2P6O2(s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. [Pbo] (02] K = [PbO2]? a K = = [02] b 1 K = [02] [PbO,]? [Pbo] [0,] d K = = [PbO]*[O2] e The reaction for the decomposition of carbonyl bromide gas is shown below. What is the Kp for this reaction, expressed using standard units? COBr2 (g) = CO(g) + Br2 (g) Kc = 0.190 at 73°C Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 0.190 b 1.15 5.47 d 15.7 e 540.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 69E: Old-fashioned smelling salts consist of ammonium carbonate, (NH4)2CO3. The reaction for the...

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Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: CH3CO2HAceticacid+C2H5OHEthanolCH3CO2C2H5Ethylacetate+H2OK=2.2 For the following mixtures (a-d), will the concentration of H2O increase, decrease, or remain the same as equilibrium is established? a. [CH3CO2C2H5] = 0.22M, [H2O] = 0.10M, [CH3CO2H] = 0.010 M, [C2H5OH] = 0.010 M b. [CH3CO2C2H5] = 0.22 M, [H2O] = 0.0020 M, [CH3CO2H] = 0.0020 M, [C2H5OH] = 0.10 M c. [CH3CO2C2H5] = 0.88 M, [H2O] = 0.12 M, [CH3CO2H) = 0.044 M, [C2H5OH] = 6.0 M d. [CH3CO2C2H5] = 4.4 M, [H2O] = 4.4 M, [CH3CO2H] = 0.88 M, [C2H5OH] = 10.0 M e. What must the concentration of water be for a mixture with [CH3CO2C2H5] = 2.0M, [CH3CO2H] = 0.l0 M, and [C2H5OH] = 5.0 M to be at equilibrium? f. Why is water included in the equilibrium expression for this reaction?
The only stress (change) that also changes the value of K is a change in temperature. For an exothermic reaction, how does the equilibrium position change as temperature increases, and what happens to the value of K? Answer the same questions for an endothermic reaction. If the value of K increases with a decrease in temperature, is the reaction exothermic or endothermic? Explain.
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.
The formation of ammonia from its elements is an important industrial process. 3 H2(g) + N2(g) 2 NH3(g) 1. Does the reaction shift to the right or to the left, or does it remain unchanged, when extra H2 is added? (a) shift left (b) shift right (c)unchanged
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?
a. Using the free energy profile for a simple one-step reaction, show that at equilibrium K = kf/kr, where kf and kr, are the rate constants for the forward and reverse reactions. Hint: Use the relationship G = RT ln(K) and represent kf and kr, using the Arrhenius equation.(K=AeEa/RT) b. Why is the following statement false? A catalyst can increase the rate of a forward reaction but not the rote of the reverse reaction.
The equilibrium constant (Kc) for this reaction is 5.0 at a given temperature. CO(g)+H2O(g)CO2(g)+H2(g) (a) On analysis, an equilibrium mixture of the substances present at the given temperature was found to contain 0.20 mol of CO, 0.30 mol of water vapor, and 0.90 mol of H2 in a liter. How many moles of CO2 were there in the equilibrium mixture? (b) Maintaining the same temperature, additional H2 was added to the system, and some water vapor was removed by drying. A new equilibrium mixture was thereby established containing 0.40 mol of CO, 0.30 mol of water vapor, and 1.2 mol of H2 in a liter. How many moles of CO2 were in the new equilibrium mixture? Compare this with the quantity in part (a), and discuss whether the second value is reasonable. Explain how it is possible for the water vapor concentration to be the same in the two equilibrium solutions even though some vapor was removed before the second equilibrium was established.
For the endothermic reaction AB(g)A(g)+B(g), the following represents a reaction container at two different temperatures. Which one (I or II) is at the lower temperature?
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.
Old-fashioned smelling salts consist of ammonium carbonate, (NH4)2CO3. The reaction for the decomposition of ammonium carbonate (NH4)2CO3(s)2NH3(g)+CO(g)+H2O(g) is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?
The decomposition of NH4HS NH4HS(s) NH3(g) + H2S(g) is an endothermic process. Using Le Chateliers principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?
Heating a metal carbonate leads to decomposition. BaCO3(s) BaO(s) + CO2(g) Predict the effect on the equilibrium of each change listed below. Answer by choosing (i) no change, (ii) shifts left or (iii) shifts right. (a) add BaCO3 (b) add CO2 (c) add BaO (d) raise the temperature (e) increase the volume of the flask containing the reaction