I Review | Constants | Periodic TableI2 is considerably more soluble in CC4 (1) than it is inH20(1). At a certain temperature, the concentrationof I2 in its saturated aqueous solution is1.300 x 10-3 M, and the equilibrium achieved whenI2 distributes itself between H20 and CC4 isPart AI2 (aq) = I2 (CC14), K=85.5A 13.0-mL sample of saturated I2 (aq) is shaken with 13.0 mL of CCl4. After equilibrium is established, the two liquid layers areseparated. How many milligrams of I2 will be in the aqueous layer?Express your answer to two significant figures and include the appropriate units.

Given: The concentration of I2 is 1.300 x 10-3 M The volume of the sample of saturated I2 (aq) is…

I2 is considerably more soluble in CCL4 (1) than it is in H20(1). At a certain temperature, the concentration of I2 in its saturated aqueous solution is 1.300 x 10-3 M, and the equilibrium achieved when I2 distributes itself between H2O and CCl4 is Part A I2 (aq) = 12 (CC14), K=85.5 A 13.0-mL sample of saturated I2 (aq) is shaken with 13.0 mL of CC14 . After equilibrium is established, the two liquid layers are separated. How many milligrams of I2 will be in the aqueous layer? Express your answer to two significant figures and include the appropriate units.

I2 is considerably more soluble in CCL4 (1) than it is in H20(1). At a certain temperature, the concentration of I2 in its saturated aqueous solution is 1.300 x 10-3 M, and the equilibrium achieved when I2 distributes itself between H2O and CCl4 is Part A I2 (aq) = 12 (CC14), K=85.5 A 13.0-mL sample of saturated I2 (aq) is shaken with 13.0 mL of CC14 . After equilibrium is established, the two liquid layers are separated. How many milligrams of I2 will be in the aqueous layer? Express your answer to two significant figures and include the appropriate units.

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

How could I find this using the given information ?
calculate the value of the equilibrium constant, Rc₂ Q (g) + x (g) = 2 M(g) + N(0) given that KC₁ - 3.20 ког = 0.443 14.0 Кез Meg) = 2(g) 6Rcg) = 2 N(g) + 47 (8) 3 X (9) +30)(9) — 9R(g) R= ? GIVE EXPLAINED HANDWRITTEN ANSWER
6B.4(b) The equilibrium constant for the reaction N2(g) + O2(g)=2 NO(g) is 1.69×10-3 at 2300 K. A mixture consisting of 5.0 g of nitrogen and 2.0 g of oxygen in a container of volume 1.0 dm³ is heated to 2300 K and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium.20
(a) Formulate the equilibrium expression for the endo- thermic reaction AgCl-NH3(s) = A£CI(s) + NH3(g) (b) What is the effect on PNH, at equilibrium if addi- tional AgCl(s) is added? (c) What is the effect on PNH, at equilibrium if addi- tional NH3(g) is pumped into or out of the system, provided that neither of the two solid phases shown in the chemical equation is completely used up? (d) What is the effect on PNH; of lowering the temperature?
Write the reaction quotient, Qc, and the equilibrium constant, Kc, for 2C3H8(g) + 10O2(g) ⥫⥬ 6CO2(g) + 8H2O(g)
Please don't provide hand written solution.....
please don't provide handwrittin solution....
Use the data in the supporting materials to calculate the equilibrium constant (Kp) for the following reaction at 25°C. 2 SO2(g) + O2(g) =2 S03(g) Кра 4.24e24 Calculate Kp for the reaction at 49°C using the following equations. (a) the van't Hoff equation below. (P), A,H° RT? a In K Кр = 1.138e22 (b) the Gibbs-Helmholtz equations below to find A-G° at 49°C and hence, Kp at the same temperature. AG ΔΗ (i) = - T2 A-G2 A;G1 1 (ii) T2 T1 T1 Kp = 1.138e22 (c) A-G° = ArH° – TA¡S° to find A-G° at 49°C and hence, Kp at the same temperature. Кр 3D 1.7742е22 State the approximations employed in each case. The assumption that A,H° is temperature independent and equal to the value calculated at 298.15 K is required by all three parts A second assumption that AS° is temperature independent and equal to the value calculated at 298.15 K is required by part (c) Compare your results. The answers calculated in parts (a) and (b) ▼ in part (c) are very close as expected because the formulas used to…
Consider the following reactions: CO (g) + H2O (g) <-> CO2 (g) + H2 (g) | Kp(1)= 0.694 at 1200.K C3H8 (g) + 3 H2O (g) <-> 3 CO (g) + 7 H2 (g) | Kp(2)= 8.175 x 1015 at 1200.K Write the overall equation for the reaction of propane and steam to produce carbon dioxide and hydrogen. Calculate Kp for the overall process at 1200. K. What molecule(s) in the steps are reaction intermediate(s)? If 0.500 atm of CO2, H2, C3H8, and H2O are initially placed in the same container, then given your answer in part a., determine which direction the reaction will shift in order to establish equilibrium.
A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 °C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the sameconditions.(a) Which acid has the larger equilibrium constant for ionizationHA [HA(aq) ⇌ A−(aq) + H+(aq)] or HB [HB(aq) ⇌ H+(aq) + B−(aq)] ?(b) What are the equilibrium constants for the ionization of these acids?
The equilibrium constant Kc for C + CO2 <=> 2CO is 1.9 at 1000 K and 0.133 at 298K. Is the reaction endothermic or exothermic?
Give correct detailed Solution