L_{2} is considerably more soluble in CC*L_{4}(1) than it is in H_{2}*O(1) At a certain temperature, the concentration of I_{2} in its saturated aqueous solution is 1.3*10^-3* M and the equilibrium achieved when I_{2} distributes itself between H_{2}*O and CC*L{4} is 12 (aq) rightleftharpoons 1 2 (CCL 4),; K = 85.5Part A: A 12.0-mL sample of saturated I_{2}(aq) is shaken with 12.0 mL of CC*L_{4} After equilibrium is established, the two liquid layers are separated. How many milligrams of will be in the aqueous layer? I_{2}

L_{2} is considerably more soluble in CCL_{4}(1) than it is in H_{2}O(1) At a certain temperature, the concentration of I_{2} in its saturated aqueous solution is 1.310^-3 M and the equilibrium achieved when I_{2} distributes itself between H_{2}O and CCL{4} is 12 (aq) rightleftharpoons 1 2 (CCL 4),; K = 85.5Part A: A 12.0-mL sample of saturated I_{2}(aq) is shaken with 12.0 mL of CC*L_{4} After equilibrium is established, the two liquid layers are separated. How many milligrams of will be in the aqueous layer? I_{2}

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

A mixture of 0.450 M H2, 0.473 M I2, and 0.926 M HI is enclosed in a vessel and heated to 430 °C. H2(g)+I2(g)↽−−⇀2HI(g)?c=54.3 at 430 ∘C Calculate the equilibrium concentrations of each gas at 430 ∘C .
For the following reaction: A(aq) + 2 B(ag) = 2 C(ag) + 2 D(ag) Calculate the magnitude of Ke (don't report the units) assuming the following composition at equilibrium: [A] = 0.339 mol L-1 [B] = 0.864 mol L-1 [C] = 0.476 mol L-1 [D] = 0.163 mol L-1 %3D
At 25 ºC HCl(g) H2(g) + Cl2(g) Kc = 3,2.10-34 If a 1.0 L flask is filled with HCl under 0.22 bar, what are the partial pressures of HCl, H2 and Cl2 at equilibrium?
2 HBr(g) ↔ H2(g) + Br2(g) this reaction has an equilibrium constant Kp = (8.5x10^-5). If the equilibrium partial pressure of H2(g) is (7.22x10^-1) bar and Br2(g) is (4.02x10^0) bar, what the is equilibrium partial pressure of HBr in bar?
Give detailed Solution with explanation (don't give Handwritten answer
At a particular temperature, Kc=6.5x10^-2 for
18. Given these equilibrium expressions for the dissolution of CO2 gas in water: CO2(aq)+H2O(1) H2CO3(aq) H2CO3(aq)+ H2O(1)HCO3(aq) + H3O*(aq)
Balance each of the following examples of heterogeneousequilibria and write its reaction quotient, Q꜀:
At a particular temperature, Kc=1.6x10^-2 for
When 18.0 mL of a 7.32x10*M iron(III) nitrate salution is combined with 15.0 ml. of a 5.10×10M ammonium sulfide solution dnes a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q is equal to
Give a clear handwritten answer of all sub parts reaction..?
At a certain temperature , the given reaction has an equilibrium constant of K_{p} = 363; PCl 3 (g)+Cl 2 (g) rightleftharpoons PCl 5 (g); PC*l_{5} is placed in a sealed container at an initial pressure of 0.0640 bar. What is the total pressure at equilibrium ? Use the quadratic formula in solving steps.