The reaction 2 SO2(g) + O2(g) 2 SO3(g) is at equilibrium at 543K. Before the reaction, the concentrations of the gases were [SO2] = 0.060 mol/L, [O2] = 0.050 mol/L, and [SO3] = 0.00 mol/L. At equilibrium, [SO3]=0.040 mol/L. %3D What are the K. and the K, values? (R = 0.08206 atm-L/mol-K) %3D OK= 8.88; K,= 0.200 %3D OK= 133; K,= 2.98 %3D OK= 13.3; K,= 0.325 O K= 4.0; K,= 0.090 %3D

The reaction 2 SO2(g) + O2(g) 2 SO3(g) is at equilibrium at 543K. Before the reaction, the concentrations of the gases were [SO2] = 0.060 mol/L, [O2] = 0.050 mol/L, and [SO3] = 0.00 mol/L. At equilibrium, [SO3]=0.040 mol/L. %3D What are the K. and the K, values? (R = 0.08206 atm-L/mol-K) %3D OK= 8.88; K,= 0.200 %3D OK= 133; K,= 2.98 %3D OK= 13.3; K,= 0.325 O K= 4.0; K,= 0.090 %3D

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...

See similar textbooks

Similar questions

For the reaction H2(g) + Br2(g) =2 HBr(g), Kc = 81.4 at 385°C. If [H2] = [Br2] = [HBr] = 2.4 x 10-4 M at 385°C, which one of the following is correct? %3D [HBr] increases as the system approaches equilibrium. [H2] and [HBr] decreases as the system moves toward equilibrium. [H2] and [Br2] increases as the system approaches equilibrium. There is not enough information given to make a determination. [HBr] and [Br2] increases as the system approaches equilibrium. The system is at equilibrium.
Consider the following equilibrium reaction: 2NO (g) + Cl2 (g) 2 NOCl (g) K=12 At equilibrium, [NOCl] = 1.60 M and [NO] = 0.80 M. The [Cl2] is
A sample of HI was placed in a container and the following reaction was allowed to come equilibrium. H₂(g) + 1₂(g) = 2 HI(g) The equilibrium concentrations were found to be [HI] = 3.88 M and [H₂] = [1₂] = 0.556. Calculate the equilibrium const Kc, for the reaction. Note Kc is often called K.
A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont
following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present, calculate the equilibrium partial pressures of H2(g), O2(g), and H2O2(g).
An equilibrium reaction has a K = 3.2 x 10-4. What can be said about the reaction? [Reactants] [Products] [Reactants]> [Products] [Reactants] [Products] < =
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
6. Hydrogen gas is finding more acceptance as an alternative fuel. It is produced along with carbon dioxide by the reaction of carbon monoxide and gaseous water at 915 K. At this temperature, the equilibrium constant (K.) is 1.56. If this reaction is started in a 4.00 L closed system flask with 0.450 mol of CO, 1.25 mol H2O, 1.15 mol CO2, and 3.50 mol H2, calculate the concentrations of all substances in the flask initially and at equilibrium. Put these values in the ICE table below. (Hint: you will need to use the quadratic formula.) CO Н20 CO2 H2 INITIAL CHANGE EQUILIBRIUM 0.1125 0.3125 0.2875 0.875 -X -X +X +x e these values in the table. d. Calculate the reaction quotient, Q. e. Express the direction of equilibrium shift as an algebraic expression. Complete the change row of the table. f. Substitute the algebraic expressions into the equilibrium expression and solve for the equilibrium concentrations. Place these values in the table.
Consider the following equilibrium process at 686 degrees celsius. CO2 (g) + H2 (g) ---> CO (g) + H2O (g) The equilibrium concentrations of the reaction species are [CO]= 0.0510 M, [H2]= 0.0410 M, [CO2]= 0.0840 M, and [H2O]= 0.0390 M. a) alculate Kc for the reaction at 686 degrees celcius. Round your answer to 3 significant figures. b) If we add CO2 to increase its concentration to 0.420 M, what will the concentration of all the gases be when equilibrium is reestablished? [CO2]= M. Round your answer to 3 significant figures. c) [H2] = M. Round your answer to 2 significant figures. d) [CO]= M. Round your answer to 2 significant figures. e) [H2O]= M. Round your answer to 2 significatnt figures
3. Given the reaction: 2NH3(g) → N2(g) + 3H2(g)Determine the Kc of the reaction at 472°C if the equilibrium concentrations were determined to be[H2] = 0.1270 M[N2] = 0.04020 M[NH3] = 0.002720 M