MAI Van JL.cas-Cudo Lab Assignment #3 E.mheducation.com Saved # 3 6 Be sure to answer all parts. Consider the following equilibrium system involving SO2, Cl2, and SO,Cl, (sulfuryl dichloride): SO2(g) + Cl2(g) = SO,C(g) Predict how the equilibrium position would change if the following changes were to occur. The temperature remains constant in each case. (a) Cl, gas is added to the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. ((More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (b) SO,Cl, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (c) SO, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) < Prev 7 of 10 Ne > Next MacBook/

MAI Van JL.cas-Cudo Lab Assignment #3 E.mheducation.com Saved # 3 6 Be sure to answer all parts. Consider the following equilibrium system involving SO2, Cl2, and SO,Cl, (sulfuryl dichloride): SO2(g) + Cl2(g) = SO,C(g) Predict how the equilibrium position would change if the following changes were to occur. The temperature remains constant in each case. (a) Cl, gas is added to the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. ((More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (b) SO,Cl, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (c) SO, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) < Prev 7 of 10 Ne > Next MacBook/

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Suppose a 500. mL flask is filled with 0.90 mol of NO, 1.6 mol of NO and 1.4 mol of CO,. The following reaction becomes possible: NO,(g) + CO (g) = NO (g)+ CO,(g) The equilibrium constant K for this reaction is 3.12 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. IM
O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 2.0 mol of NO, and 1.3 mol of NO. The following reaction becomes possible: NO, (g) + NO(g) → 2NO, (g) The equilibrium constant K for this reaction is 6.91 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Explanation Check 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use |P 21
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General Chemistry 4th Edition McQuarrie Rock Gallogly An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) = CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂: University Science Books presented by Macmillan Learning »))) R. mol
. Consider the equilibrium 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H₂O(g). Predict the effect on the equilibrium concentration by the addition of N₂. A The equilibrium will shift to produce more nitrogen. B The equilibrium will shift to produce more reactants. C The equilibrium will shift to produce more products. D The reaction is already at equilibrium. E None of the above Given: 2P(g) + 3Cl2(g) → 2PC13(g) K Calculate the equilibrium constant for the following reaction. P(g) + 3/2Cl2(g) → PCI(g) AK BK¹ C 2K D 0.5K EK¹/2
Consider the equilibrium reaction below: N₂(g) + O₂(g) 2 NO(g) Create an equilibrium constant, K, expression for the above reaction using the drag and drop tools: K= [N₂][0₂] [N₂]+[0₂] [NO]² [N]²[O]² [NO] 2[NO]
Suppose a 500.mL flask is filled with 1.0mol of Cl2 , 1.3mol of CHCl3 and 0.50mol of CCl4 . The following reaction becomes possible: +Cl2gCHCl3g +HClgCCl4g The equilibrium constant K for this reaction is 1.32 at the temperature of the flask. Calculate the equilibrium molarity of CHCl3 . Round your answer to two decimal places.
O KINETICS AND EQUILIBRIUM Try again. 2/5 Calculating equilibrium composition from an equilibrium constant Try Again Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible: N,(g) +0,(2) – 2No(2) The equilibrium constant K for this reaction is 5.01 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. 3.36 M II
Consider the following equilibrium: NH3(g) + HCl(g) NH4CI(s) Suppose a vessel containing NH4Cl(s), NH3(g) and HCl(g) is at equilibrium. If the volume of the vessel is instantaneously doubled while keeping the temperature constant, when a new equilibrium is reached, which of the following statements is incorrect? The partial pressures of NH3 and HCI in the vessel remain unchanged. The total pressure is halved. O The value of Kp remains unchanged. O The number of moles of NH4Cl decreases. O The amount of NH3 and HCI doubles.