please help with both, will upvote 1] me CH₂Cl₂ is placed in a sealed flask and heated to 408 K. When equilibrium is reached, the flask is found to contain CH₂Cl₂ (1.16×10-2 M), CH4 (1.77x10-2 M), and CCl4 (3.20x10-2 M). What is the value of the equilibrium constant for this reaction at 408 K? 2CH₂Cl₂(g) CH4(g) + CCl4(g) K = 2] Question Content Area The equilibrium constant, K, for the following reaction is 1.29x10-² at 600 K. CoCl₂(g) = CO(g) + Cl2₂(g) If an equilibrium mixture of the three gases in a 12.3 L container 600 K contains 0.459 mol of COCl₂(g) and 0.388 mol of CO, the equilibrium concentration of Cl₂ is M.

please help with both, will upvote 1] me CH₂Cl₂ is placed in a sealed flask and heated to 408 K. When equilibrium is reached, the flask is found to contain CH₂Cl₂ (1.16×10-2 M), CH4 (1.77x10-2 M), and CCl4 (3.20x10-2 M). What is the value of the equilibrium constant for this reaction at 408 K? 2CH₂Cl₂(g) CH4(g) + CCl4(g) K = 2] Question Content Area The equilibrium constant, K, for the following reaction is 1.29x10-² at 600 K. CoCl₂(g) = CO(g) + Cl2₂(g) If an equilibrium mixture of the three gases in a 12.3 L container 600 K contains 0.459 mol of COCl₂(g) and 0.388 mol of CO, the equilibrium concentration of Cl₂ is 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

The equilibrium expression for the the reaction:H2(g) + I2(g) <--> 2HI(g) would be: Given the reaction: A + B <--> C + DThe concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (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
For the following hypothetical equilibrium, what is the value of the equilibrium constant (Keq) if the concentrations at equilibrium are: [A] = 4.5×10–5; [B]=2.2×10–2 and [C] = 9.4×10–3. A (g) + 2 B (g) <-> C (g) choose only one option and explain
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? |
The equilibrium constant for the following reaction is 0.18 at a set temperature. Find the equilibrium concentrations if the initial concentration of PCl3 is 0.225 mol/L and the initial concentration of Cl2 is 0.150 mol/L. PCI3(g)+CI2(g)=PCI5(g)
6. On analysis, an equilibrium mixture for the reaction: 2 H,S( ) was found to contain 1.0 mol H,S, 20.0 mol H, and 0.80 molS, in a 4.0 L vessel. Calculate the equilibrium constant (Kc) for this reaction. 2 H,(g) + S,(g) 2' 51 80 O 13 29 3
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?
2NO(g) + Br₂(g) ⇒ 2NOBr(g) 4.000 mol of each reactant was added to a rigid 2.000 L container. At equilibrium, the concentration of Br2 is 1.357 M. What is the equilibrium constant for the reaction? Kp = [?] KE Enter
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.…
The equilibrium-constant of the reaction NO2 (g) + NO3(g) = N2O5 (g) is K = 2.1 x 10-20. What can be said about this reaction? • View Available Hint(s) At equilibrium the concentration of products and reactants is about the same. At equilibrium the concentration of products is much greater than the concentration of reactants. At equilibrium the concentration of reactants is much greater than that of products. O There are no reactants left over once the reaction reaches equilibrium.
Question 13 of 50 Consider the equilibrium system described by the chemical reaction below. When 1.50 mol of CO, and an 10.0 mol solid carbon are heated in a 20.0 L container at 1100 K, the equilibrium concentration of CO is 0.0700 M. Determine the concentrations of all species at equilibrium and then calculate the value of Kc for 2 this reaction. C(s) + CO,(g) =2 CO(g) 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C(s) CO,(9) 2 СО(g) + Initial (M) Change (M) Equilibrium (M) 5 RESET 1.50 10.0 20.0 0.500 0.150 0.0750 0.0700 -0.0700 0.140 -0.140 0.0350 -0.0350 0.110 0.0400 0.0050 1L
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 510 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 7.99 L container at 510 K contains 0.377 M PCl5, 8.23×10-2 M PCl3 and 8.23×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 18.5 L? [PCl5] = M [PCl3] = M [Cl2] = M