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 13.0 mL The value of K is 85.5 The molar mass of I2 (iodine) is 253.81 g/molUsing the concentration and volume of I2 (aq), the number of moles of I2 (aq) before mixing will be: nI2aq=concentration×volume=1.300×10-3 M×13.00 mL×1 L1000 mL=1.69×10-5 mol Here, the sample of saturated I2 (aq) is shaken with 13.0 mL of CCl4. Let us assume that the number of moles of I2 in the CCl4 phase is x mol and the number of moles of I2 in the aqueous phase is (1.69 x 10-5 - x) mol at equilibrium. In terms of K (distribution coefficient), the expression is classified as follows: K=I2 CCl4I2 (aq) [I2 (CCl4)] is the equilibrium concentration of I2 in the CCl4 phase [I2 (aq)] is the equilibrium concentration of I2 in the aqueous phase Now solving the equation and give: 85.5=x mol13.0 mL1.69×10-5 -x mol13.0 mL85.5=x1.69×10-5 -x x=0.00144495-85.5x86.5x=0.00144495 solving the equation further and gives: x=1.67×10-5 Now the number of moles of I2 in the aqueous phase will be (1.69 x 10-5 - 1.67 x 10-5) mol = 2 x 10-7 mol Using the number of moles of I2 (aq) and molar mass of iodine, the mass of I2 will be: Mass of I2= molar mass×number of moles=253.81 g/mol×2×10-7 mol=5.08×10-5 g=5.1×10-2 mg Hence, 5.1 x 10-2 milligrams of I2 will be in the aqueous layer.

Science

Chemistry

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

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
Please don't provide hand written solution.....
please don't provide handwrittin solution....
-2 The equilibrium constant, K, for the following reaction is 1.71x10 at 1120 K 25O₂(g) 250₂(g) + O₂(9) Calculate K, at this temperature for the following reaction SO₂(g) SO₂(g) + 1/2O₂(g)
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.
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?