1) Consider the following reaction occurs: 3 Al2Cls (g) 2 Al3Cls (g) a) In an experiment at 454 K, the equilibrium concentration of Al2Cls is 0.000167 M and the equilibrium concentration of Al3Cls is 0.0141M. Calculate K for the reaction. b) A 1.00 L flask is charged with 0.00513 moles of Al2Cl6 at 454 K and allowed to establish equilibrium (in other words, is held at T until equilibrium is established). Estimate, to three significant figures, the molar concentrations, mol/L (M), of both species after the system has attained equilibrium.

1) Consider the following reaction occurs: 3 Al2Cls (g) 2 Al3Cls (g) a) In an experiment at 454 K, the equilibrium concentration of Al2Cls is 0.000167 M and the equilibrium concentration of Al3Cls is 0.0141M. Calculate K for the reaction. b) A 1.00 L flask is charged with 0.00513 moles of Al2Cl6 at 454 K and allowed to establish equilibrium (in other words, is held at T until equilibrium is established). Estimate, to three significant figures, the molar concentrations, mol/L (M), of both species after the system has attained equilibrium.

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

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.
At a certain temperature, the equilibrium constant K for the following reaction is 352.: H,(g) + Cl,(g) 2HC1(g) Use this information to complete the following table. Suppose a 17. L reaction vessel is filled with 0.38 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little H2 and Cl2 There will be very little HCI. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K =0 2 HCl(g) H,(9)+Cl,(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = | 2 H,(9)+2C12(9) 4 HCl(g)
The equilibrium constant, K. , for the following reaction is 5.10×10-6 at 548 K. NHẠC(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 7.80 L container at 548 K contains 2.74 mol of NH,Cl(s) and 0.323 mol of NH3, the number of moles of HCl present is moles.
The equilibrium constant, K, for the following reaction is 1.20x10-2 at 500K. PCI5(g) PCI3(g) + Cl2(g) If an equilibrium mixture of the three gases in a 15.3 L container at 500K contains 0.359 mol of PCI5(g) and 0.228 mol of PC13, the equilibrium concentration of Cl2 is М.
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
SC At a certain temperature, the equilibrium constant K for the following reaction is 506.: Br₂(g) + OC1₂(g) BrOCI(g) + BrCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 0.62 mol of Br₂ and 0.62 mol of OCI₂. What can you say about the composition of the mixture in the vessel at equilibrium? ! 1 What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. BrOCI(g)+BrCl(g) Q A What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 Br₂(9)+20C1₂(9) P 2 BrOCI(g)+2BrCl(9) Explanation NO 2 W S Check *3 # E Br₂(9)+OCL₂(9) D D DS 4 C R F % LO 5 O There will be very little Br₂ and OCl₂. O There will be very little BrOCI and BrCl. ONeither of the above is true. K = 0 K = 0 T MacBook Pro 20 ^ 6 G Y C & 7 H 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy C U 00 8 J X I ( 9 K 0 0 < F
consider the reaction h2(g) + f2(g) 2hf(g) with the equilibrium constant k = 100. at some temperature. a) how many moles of h2(g) must be mixed with 1.00 moles of f2(g) in a 1.00 I high-pressure flask to produce 1.70 moles of hf(g) once the flask reaches equilibrium?
Phosphorus pentachloride decomposes according to the chemical equation PCI,(g) = PCI, (g) + CL(g) K. = 1.80 at 250 C A 0.1385 mol sample of PCI, (g) is injected into an empty 2.15 L reaction vessel held at 250 C. Calculate the concentrations of PCI,(g) and PCI, (g) at equilibrium. [PCI, ] = [PCI,] = %3D rity Science Bok
A student ran the following reaction in the laboratory at 325 K: 2NO(g) + Br2(g) 2NOBr(g) When she introduced 0.102 moles of NO(g) and 9.44x10-2 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBR(g) to be 7.16x10-2 M. Calculate the equilibrium constant, Ke, she obtained for this reaction.
Nitric oxide, NO, reacts readily with chlorine gas as follows: 2NO(+ Cl2(g) 2NOCI(g) At 700 K, the equilibrium constant, K, for the reaction is 0.26. Are the following mixtures of NO, Cl₂ and NOCI at equilibrium? If not, predict the direction in which the reaction will proceed. [NOCI] = 0.11 M a.) [NO] = 0.15 M b.) [NO] = 0.15 M c.) [NO] = 0.12 Man [Cl₂] = 0.31 M, [Cl₂] = 0.20 M [Cl₂] = 0.10 M [NOCU] = 0.051 M I [NOCU] = 0.050 M
The equilibrium constant, K, for the following reaction is 5.10x10 at 548 K. NH4Cl(s) NH3(g) + HCI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.368 mol NH4Cl, 2.26x10-3 M NH₂ and 2.26×10-³ M HCl. If the concentration of HCl(g) is suddenly increased to 3.22×103 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH₂] = [HCI] M M
A mixture consisting of 0.2000 mol CO2, 0.1000 mol Hz and 0.1600 mol H20 is placed in a 2.00- L vessel. The following equilibrium is established: CO2(amt H2(g) co(g) + H20(g) At equilibrium, [H20] = 0.0856 M. a) What are the equilibrium concentrations of CO2, H2 and CO? b) Calculate kKe for the reaction.