Phosphorus pentachloride decomposes according to the following equation. PCI 5(9) PC13(g) + Cl₂(g) Kc = 0.0136 What are the concentrations (in M) of PCI 5, PCI 3, and Cl₂ in an equilibrium mixture produced by the decomposition of a sample of pure PCI5 with an initial [PCI5] of 1.92 M? Hint: you will need the quadratic formula or method of successive approximations (see Appendix A1.4 for review if needed) [PCI 5] M [PCI 3] M [Cl₂] = = = M

Phosphorus pentachloride decomposes according to the following equation. PCI 5(9) PC13(g) + Cl₂(g) Kc = 0.0136 What are the concentrations (in M) of PCI 5, PCI 3, and Cl₂ in an equilibrium mixture produced by the decomposition of a sample of pure PCI5 with an initial [PCI5] of 1.92 M? Hint: you will need the quadratic formula or method of successive approximations (see Appendix A1.4 for review if needed) [PCI 5] M [PCI 3] M [Cl₂] = = = M

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

MISSED THIS? Read Section 16.8 (Pages 701 - 710); Watch KCV 16.8, IWE 16.9. Consider the following reaction and associated equilibrium constant: aA (g) + bB (g) = cC (g) Kc = 3.0 Part A Find the equilibrium concentrations of A, B, and C for a = 1, b = 1, and c = 2. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction. Express your answer using two significant figures. Enter your answers separated by commas. [A], [B]. [C] = Submit Part B X Incorrect; Try Again; 3 attempts remaining IV—| ΑΣΦ 5 Previous Answers Request Answer [A], [B], [C] = Submit Find the equilibrium concentrations of A, B, and C for a = 1, b = 1, and c = 1. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction. Express your answer using two significant figures. Enter your answers separated by commas. OF IVE ΑΣΦ Request Answer ? www M ? M
Question 2, part c: please see attached Part a answer:if an initial concentration before equilibrium of c2h4o2 is 0.080 M, what are the equilibrium conc of the three species in the equilibrium:[H3O+]=[C2H3O2-]=1.20x10^-3M Part b answer: a solution in which this reaction takes place is analyzed and found to have [C2H4O2]=0.073M and [C2H3O2-]=0.251M and pH 2.131. Is the system and equilibrium? Calculate QQc=2543.0 x 10^-5Kc=1.81 x 10^-5 not at equilibrium
The equilibrium constant, Kc, for the following reaction is 7.00 × 10-5 at 673 K. NH₂I(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 5.72 L container at 673 K contains 2.94 mol of NHI(s) and 0.409 mol of NH3, the number of moles of HI present is mol.
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.362 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] M [H2] M [12] M
Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One way to represent this equilibrium is: 2 AlBr3(s)2 Al(s) + 3 Br2(1) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) AIBr3(s) PAl(s) + 3/2 Br2(1) K1 = 2) Al(s) + 3/2 Br2(1) AlBr3(s) K2 = 3)2 Al(s) + 3 Br2(1) =2 AIBR3(s) K3 = Drag and drop your selection from the following list to complete the answer: (1/K)1/2 K/2 1/K
K= 6-7 x 10 3. Consider the reaction: P 2NO2(g) + Cl2(g) 2NOCI The initial pressure of NO, was 1.577 atm and the initial pressure of Cl₂ was 0.427 atm. At equilibrium, the partial pressure of NOC1 is 0.624 atm. Calculate K.
Question 41 of 44 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 7.1 x 10 at a certain temperature. If a solid sample of CaCrO4 dissolves in solution, what will the equilibrium concentration of Ca in the solution be? CaCrO.(s)= Ca (aq) + CrO (aq) NEXT Based on the given values, set up ICE table in order to determine the unknown. CaCrO-(s) Ca-(aq) CrO. (aq) Initial (M) Change (M) +2x +2x Equilibrium (M) 7.1 x 10-2x +2x +2x RESET 7.1 x 10 +2x -2x 7.1 x 10 +* 7.1 x 10-r 7.1x 10+ 2x 7.1x 10-2x
Question 2, part c: please see attached Part a answer: if an initial concentration before equilibrium of c2h4o2 is 0.080 M, what are the equilibrium conc of the three species in the equilibrium: [H3O+]=[C2H3O2-]=1.20x10^-3M Part b answer: a solution in which this reaction takes place is analyzed and found to have [C2H4O2]=0.073M and [C2H3O2-]=0.251M and pH 2.131. Is the system and equilibrium? Calculate Q Qc=2543.0 x 10^-5 Kc=1.81 x 10^-5 not at equilibrium
C2,H2905S- (ag) + NH,CI (ag) → C2,H29O5SH (ag) + NH3 (aq) Yellow Blue Reaction after it reaches equilibrium appears Green A. Assume the reaction mixture is at equilibrium, appearing green in color, and at room temperature before each of the following disturbances. Explain which direction the reaction shifts to re-establish equilibrium and predict how the color of the solution will change 1.100 mL of water, H2O is added to the reaction mixture. 2. Solid platinum, Pt, is added to the reaction mixture. It reacts with NH3 to form N and H2 gasses. B. When the green reaction mixture at equilibrium is heated the color changes to green-blue, and then eventually, a dark blue color. When the green reaction mixture at equilibrium is placed in an ice water bath the solution color changes to a yellow-green, and eventually a bright yellow color. Is the reaction exothermic or endothermic? |
Which is the correct equilibrium constant expression for the following reactiont OK Fez Os(s) + 3H2(g) +2 Fe(s) + 3H2O(g) = [Fe2O3][H2] [Fe][H2O3 OK [Fe][H2O3 = [Fe2O3][H2]3 OK [H2O] = [H2] K OK = [Fe][H2O] [Fe2O3] [H2] [H2O] 3 H23
Consider the general reaction below. 2A(g) + B₂(g) = 2AB(g) K = 6.4 x 10-6 @ 298 K The reaction was initiated by combining 0.70 mol A and 0.90 mol B2 in a 2.0 L container. Calculate the equilibrium concentrations of the components. What is the equilibrium concentration of AB? 10[? ] [AB] = [?] x 10¹ M
What is the equilibrium-constant expression for the following reaction?N2O4 (g) <--> 2NO2 (g)