onsider the reaction: A(g) + B(g) E--→ Cg) a) In an equilibrium mixture the following concentrations were found: A] = 0.45M, [B] = 0.63M and [C] = 0.30M. Calculate the value of the equilibrium constant for this reaction b) At the same temperature, another equilibrium mixture is analyzed and it is found that [B] = 0.21 M and [C] = 0.70 M. From this and the information above, calculate the equilibrium [A]. Answer In another equilibrium mixture at the same temperature, it is found that [A] = 0.35 M nd the [C] = 0.86 M. From this and the information above, calculate the equilibrium [B].

onsider the reaction: A(g) + B(g) E--→ Cg) a) In an equilibrium mixture the following concentrations were found: A] = 0.45M, [B] = 0.63M and [C] = 0.30M. Calculate the value of the equilibrium constant for this reaction b) At the same temperature, another equilibrium mixture is analyzed and it is found that [B] = 0.21 M and [C] = 0.70 M. From this and the information above, calculate the equilibrium [A]. Answer In another equilibrium mixture at the same temperature, it is found that [A] = 0.35 M nd the [C] = 0.86 M. From this and the information above, calculate the equilibrium [B].

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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34.
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
Consider the following system at equilibrium at 698 K. 2 HI(g)→ H₂(g) + I₂ (9) Use the References to access importa When some HI(g) is removed from the equilibrium system at constant temperature, the reaction must O run in the forward direction to reestablish equilibrium. O run in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. The concentration of H₂ will O increase. O decrease. O remain the same.
For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.220 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.
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A chem gineer is studying the following reaclon! HCN(aq)+NH,(aq) - CN (aq)+NH,(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.99. The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound concentration expected change in concentration HCN 0.84 M O t increase OI decrease O (no change) NH, 1.00 M O t increase O, decrease O (no change) CN 0.42 M O 1 increase O. decrease O (no change) NH, 0.33 M O t increase O, decrease O (no change) HCN 1.01 M O t increase O. decrease O (no change) NH, 1.17 M O t increase O. decrease O (no change) CN 0.25 NM M t increase O. decrease O (no change) NH. 0.16 MM O t increase O.…
O KINETICS AND EQUILIBRIUM 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) 2 NOCI(g) K,=2. x 107 He fills a reaction vessel at this temperature with 8.0 atm of nitrogen monoxide gas and 9.7 atm of chlorine gas. Use this data to answer the guestions 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 II
The equilibrium constant, K. , for the following reaction is 1.80x10 at 298 K. NH,HS(s) NH3(g)+ H,S(g) If an equilibrium mixture of the three compounds in a 6.85 L container at 298 K contains 1.56 mol of NH HS(s) and 0.468 mol of NH3, the number of moles of H,S present is moles.
Consider the equilibrium between SbCl5, SbCl3 and Cl₂. SbCl5(g) SbCl3(g) + Cl₂(g) K = 2.46x10-² at 530 K The reaction is allowed to reach equilibrium in a 7.30-L flask. At equilibrium, [SbCl5] = 0.430 M, [SbCl3] = 0.103 M and [Cl₂] = 0.103 M. (a) The equilibrium mixture is transferred to a 14.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.6-L flask. [SbCl5] = [SbCl3] = [Cl₂] |||| ΣΣΣ
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The equilibrium constant, K., for the following reaction is 77.5 at 600 K. CO(g) + Cl(g) COCI,(g) Calculate the equilibrium concentrations of reactant and products when 0.451 moles of CO and 0.451 moles of Cl, are introduced into a 1.00 L vessel at 600 K. [CO] [Cl] [COCL,] = MMM
Can you provide an explanation? And show the steps