Upload the answer to this question as an image. Show your working.Consider the equilibrium step in the preparation of nitrosyl chloride, NOCI.2NO(g) + Cl2(g) = 2NOCI(g)At a temperature of 727°C the equilibrium constant for this reaction is 3.09 × 10².The concentration of reactants and products at a particular moment in time in the realtion mixtureis given below.[NO] = 0.0620 mol L1, [Cl2] = 0.538 mol L-1, [NOCI] = 0.838 mol L-1(i) Calculate the reaction quotient, Q, at this particular time.(ii) State whether the system is at equilibrium. Justify your answer.(iii) If the system is not at equilibrium explain which way the system will move in order to reachequilibrium. Give a reason for your answer.

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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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Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 7.45 × 10-5: NO₂(g) + CO(g) ⇒ NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 20. L reaction vessel is filled with 1.5 mol of NO and 1.5 mol of CO₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. NO(g)+CO,(9) NO₂(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 NO₂(g) + 3 CO(g) P 3 NO(g)+ 3 CO₂(9) There will be very little NO2 and CO. There will be very little NO and CO₂. Neither of the above is true. K = 0 K = 0 x10 Ś ? ollo 18 Ar BA
Consider the equilibrium system described by the chemical reaction below For this reaction, Kc = 2.4 x 10 at a particular temperature. If the equilibrium concentrations of H2O and Hz are 0.11 M and 0.019 M, respectively, determine the concentration of Oz at equilibrium. 2 H.O(g) = 2 H2(g) + On(g) NEXT If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms. Ke = 2.4 x 10 3 O RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11F [0.019 [2x]
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A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) ⇒ C₂H₂(g) + 3 H₂ (g) K₂=1.x10-5 He fills a reaction vessel at this temperature with 15. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. O yes no atm X
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) C₂H₂(g) + 3H₂(g) K₂=6. × 10 -8 He fills a reaction vessel at this temperature with 7.0 atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. 0 yes no atm x10 X Ś
5. Consider the following equilibrium, where both the forward and reverse directions are elementary reactions. COCI (g) + Cl (g) === CO (g) +Cl2 (g) a) Write the Equilibrium Expression. b) At 298 K, the rate constants for the forward and the reverse directions are 9.3 x 10 M's¹ and 14 x 100 M's respectively. What is the value for the equilibrium constant? c) If you start with [COCI] = 1.0 M and [CI] = 0.10 M, what are the concentrations of CO and Cl₂ at equilibrium? d) Sketch a graph of the relative concentrations of reactants and products versus Time. (Be sure to label everything)
Enter your answer in the provided box. Pure phosgene gas (COCl2), 0.0290 mol, was placed in a 1.30−L container. It was heated to 830.0 K, and at equilibrium, the pressure of CO was found to be 0.507 atm. Calculate the equilibrium constant KP for the reaction. CO(g) + Cl2(g) ⇌ COCl2(g) KP =
At 700 K, the reaction 2SO,(g) + O2(g) 2SO3(g) has the equilibrium constant K = 4.3 x 106, and the following concentrations are present: [SO2] = 0.10M; [SO3] = 10. M; [02] = 0.10 M. Is the mixture at equilibrium? O There is not enough information to be able to predict the direction. O It is always at equilibrium O Yes, the mixture is at equilibrium. O No it is not at eqilibrium
Using the small x approximation to solve equilibrium problems A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO (g) + Cl, (g)=2NOCI (g) K,=4. x 10-6 He fills a reaction vessel at this temperature with 11. atm of nitrogen monoxide gas and 10. atm of chlorine gas. Use this data to answer the questions in the table below. O yes Can you predict the equilibrium pressure of NOCI, using only the tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of NOCI at right. Round your answer to 1 significant digit. atm
For the following chemical equilibrium: N2(g) + O2(g) → 2NO(g), the equilibrium constant (Kp) was experimentally determined to be 0.0017 at 2300 K. At a given point in time, the partial pressures of the gases were found to be: PN2 = 0.660 atm, Po2 = 0.660 atm, and PNO = 0.0272 atm. Which of the statements noted below is TRUE? %3! O Qp Kp, so the reaction will consume products in order to generate more reactants. O Q, = Kp, so the system is at chemical equilibrium. O The value of K, will decrease until it is equal to Qp. O The value of K, will increase until it is equal to Qp-
A chemical engineer is studying the following reaction: 2 NO(g)+2H2(g) → N,(9)+2H2O(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0038. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound pressure expected change in pressure vessel NO 7.58 atm f increase I decrease (no change) H2 8.02 atm f increase I decrease (no change) A N, 4.16 atm f increase I decrease (no change) H,0 2.79 atm f increase I decrease O (no change) NO 8.89 atm ↑ increase I decrease (no change) H2 9.33 atm f increase I decrease (no change) В N2 3.51 atm f increase I decrease (no change) H,0 1.48 atm f increase I decrease (no change) NO…

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