15.43 At 100°C, the equilibrium constant for the reaction COCI2(8) CO(g) + Cl2(g) has the value K= 2.19 x 10 10, Are the following mixtures of COCI2, CO, and Cl2 at 100 °C at equilibrium? If not, indicate the direc- tion that the reaction must proceed to achieve equilibrium. (a) [COCI2]= 2.00 x 103 M, [CO] = 3.3 x 10M, [Cl2] 6.62 x 106 M (b) [COCI2] = 4.50 x 102 M, [CO] = 1.1 x 107 M, [Cl2] 2.25 x 106 M (c) [COCI2] 0.0100 M, [CO] [Cl2] = 1.48 x 10-6 M

15.43 At 100°C, the equilibrium constant for the reaction COCI2(8) CO(g) + Cl2(g) has the value K= 2.19 x 10 10, Are the following mixtures of COCI2, CO, and Cl2 at 100 °C at equilibrium? If not, indicate the direc- tion that the reaction must proceed to achieve equilibrium. (a) [COCI2]= 2.00 x 103 M, [CO] = 3.3 x 10M, [Cl2] 6.62 x 106 M (b) [COCI2] = 4.50 x 102 M, [CO] = 1.1 x 107 M, [Cl2] 2.25 x 106 M (c) [COCI2] 0.0100 M, [CO] [Cl2] = 1.48 x 10-6 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

5) Determine the value of K for the following reaction if the equilibrium concentrations are as follows: [P4010leg = 4.000 moles, [P4leq = 4.000 moles, [O2leg = 2.000 M %3D %3D P4(s) + 5 02(g) P4010(s) 6) Determine the value of K for the following reaction if the equilibrium concentrations are as follows: [N2leq 2.25 M, [O2leg = 3.67 M, [N20]eg = 3.39 M. %3D %3D %3D 2 N20(g) = 2 N2(g) + 02(g)
please don't provide handwrittin solution....
References Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 688 K: 2HI(g) H2(g) + I½(g) When he introduced HI(g) at a pressure of 4.87 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.510 atm. Calculate the equilibrium constant, K,, he obtained for this reaction. %3D Submit Answer
At 37.0 °C, the reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) has K = 2.94x10-8. If [H2O] = 55.5 mol L-1, [H+] = 95.4 µmol L-1, and [HCO3-] = 12.4 mmol L-1 at equilibrium, determine the PCO2 (pressure of CO2) in bar.
-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)
Compare the following two reactions ("A" and "B"), with two different equilibrium constants, K: (A) Cl2 (g) + H2 (g) = 2HCI (g) K = 0.29 (B) I2 (g) + H2 (g) = 2HI (g) K = 1.6 x 1033 %3D Which of the following statements is correct? O Reaction "A" will proceed faster because the equilibrium constant, K, is larger O Reaction "B" will proceed faster because the equilibrium constant, K, is larger O Reaction "A" favors the production of products. O Reaction "B" favors the production of products. O None of these statements are correct.
Consider the following equilibria at a given temperature: ½Nalg) + J½O>(g) = NO(g) K= 6.45 x 10°, NO (g) + 1½Brz(g) = NOB((g) K= 1.40 Determine the value of the equilibrium constant for the following reaction at the same temperature: %N(g) + ½Ozlg) + ½Br2(g) = NOBr(g) OA 583 x 107 O B.3.36 x 10-18 OC4.17x 107 OD.6.45 x 10 OE 9.03 x 10
For the following equilibrium system, K = 1.39x10-11 at 298 K. F (aq) + H₂O (1) HF (aq) + OH- (aq) Assuming that you start with just F, and that no HF or OH is initially present, which of the following best describes the equilibrium system? O The forward reaction is favored at equilibrium. O The reverse reaction is favored at equilibrium. O Appreciable quantities of all species are present at equilibrium.
The equilibrium constant Ke for the reaction PCI3 (9) + Cl2 (g) = PCI, (g) equals 3.5 at 310°C. a A sample of 38.1 g of PCl; is placed in a 2.1 L reaction vessel and heated to 310°C. What are the equilibrium concentrations of all of the species? [PCI5] = | M [PCI3] = | |M [CL] = [ M
Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N2 and Og (from air). N2 (9) + O2(9) - 2NO(9) The equilibrium constant (K.) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.082 mol N, and 0.026 mol O2 per liter, what is the concentration of NO? Concentration = M
At a certain temperature K = 1.1 × 103 for the following reac=on:Fe3+(aq) + SCN–(aq) ⇌ Fe(SCN)2+(aq)a) Calculate the concentra=on of all species at equilibrium if 0.020 moles of Fe(NO3)3 is added to 1.0 L of 0.10 M KSCN (assume no change in volume upon addi=on).b) Ader equilibrium has been reached in part a, an addi=onal 0.0050 moles of Fe(NO3)2(SCN) is addedto solu=on. Calculate the new equilibrium concentra=ons of all species assuming no change in volume.
A student ran the following reaction in the laboratory at 290 K: 2NO(g)+Br2 (g) <---> 2NOBr (g) When she introduced NO (g) 0.141 moles of and 0.121 moles of Br2 (g) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 0.0665 M. Calculate the equilibrium constant, Kc she obtained for this reaction. Kc=