The equilibrium constant, K., for the following reaction is 10.5 at 350K. 2CH;Cl½(g)CH,(g) + CC14(g) If an equilibrium mixture of the three gases in a 10.6 L container at 350K contains 0.213 mol of CH2Cl2(g) and 0.327 mol of CH4, the equilibrium concentration of CCI4 |M. is

The equilibrium constant, K., for the following reaction is 10.5 at 350K. 2CH;Cl½(g)CH,(g) + CC14(g) If an equilibrium mixture of the three gases in a 10.6 L container at 350K contains 0.213 mol of CH2Cl2(g) and 0.327 mol of CH4, the equilibrium concentration of CCI4 |M. is

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

Please don't provide handwritten solution .....
The equilibrium constant, K. for the following reaction is 77.5 at 600 K. Co(g) + C,(g)=cOC»(g) Calculate the equilibrium concentrations of reactant and products when 0.231 moles of CO and 0.231 moles of Cl, are introduced into a 1.00 L vessel at 600K. [CO] M [CL] M [COCL] =| M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K.CO(g) + Cl2(g) COCl2(g)Calculate the equilibrium concentrations of reactant and products when 0.211 moles of CO and 0.211 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
Consider the following reaction where K. = 6.30 at 723 K: 2 NH3 (g) = N2 (g) + 3 H2 (g) A reaction mixture was found to contain 7.67x104 moles of NH3 (g), 2.38×102 moles of N2 (g), and 4.58×10-2 moles of H2 (g), in a 1.00 liter container. Indicate True (I) or False (F) for each of the following: ] 1. In order to reach equilibrium NH3(g) must be produced . 2. In order to reach equilibrium K. must decrease . v 3. In order to reach equilibrium N, must be consumed . 4. Qe is greater than K. |5. The reaction is at equilibrium. No further reaction will occur.
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250 ∘C A 0.1979 mol sample of PCl5(g) is injected into an empty 2.60 L reaction vessel held at 250 ∘C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
A 0.066 mol sample of formaldehyde vapor, CH₂O, was placed in a heated 500 mL vessel and some of it decomposed. The reaction is CH,O(g) = At equilibrium, the CH₂O(g) concentration was 0.060 mol L-¹. Calculate the value of Kc for this reaction? Kc = H₂(g) H2(g) + CO(g) i
A mixture of 0.5800 M CO0.5800 M CO and 0.4910 M Cl20.4910 M Cl2 is enclosed in a vessel and heated to 1000 K1000 K . CO(g)+Cl2(g)↽−−⇀COCl2(g)?c=255.0 at 1000 KCO(g)+Cl2(g)↽−−⇀COCl2(g)Kc=255.0 at 1000 K Calculate the equilibrium concentration of each gas at 1000 K1000 K . [CO]= [Cl2]= [COCl2]=
Consider the following reaction where K. = 10.5 at 350 K: 2 CH;Cl2 (g)=CH4 (g)+ CCI4 (g) A reaction mixture was found to contain 1.10x10-2 moles of CH,Cl, (g), 4.63×10-2 moles of CH4 (g), and 3.70×10² moles of CCl (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: v 1. In order to reach equilibrium CH,Cl,(g) must be produced. v 2. In order to reach equilibrium K, must decrease v 3. In order to reach equilibrium CH, must be consumed. v 4. Qc is greater than K. 5. The reaction is at equilibrium. No further reaction will occur. T
please explain and give complete answer
At a certain temperature, 0.347 mol CH, and 0.619 mol H,S are placed in a 2.50 L container. CH,(g) + 2 H, S(g)= CS, (g) + 4 H,(g) At equilibrium, 11.8 g CS, is present. Calculate K.. K. =
19. Given the following reaction: NH.CI (s) S NH3 (g) + HCI (g) AH= +42.1 kcal Suppose the above substances in the reaction are at equilibrium at 600 K in volume V and at pressure P. State whether the partial pressure of NH3 (g) will have increased, decreased, or remained the same in order to the equilibrium to be reestablished following the disturbances of the original system. Note that some solid remains in the flask at all times. Provide a one to two sentence explanation (a) The temperature of the system is increased (b) The volume of the system is increased (c) A quantity of gaseous NH3 is added. (d) A small quantity if NH4C1 is added.
Be sure to answer all parts. The equilibrium constant K, for the reaction H2(g) + I2(g) =2 HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H,, I,, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0.222 M and [HI] = 0 M. (H2leq = |0.0692 [Lleg =|0.182 [HI]eg =0.826 < Prev 18 of Microsoft Store