13. For the decomposition of calcium carbonateCACO3 (s) = CaO (s) + CO2 (g)How will the amount (not concentration) of CaCO3 (s) change with the following stresses toΔΗ175 kJthe system at equilibrium?a. CO2 (g) is removed.b. CaO (s) is added.c. The temperature is raised.d. The volume of the container is decreased.

Given reaction: CaCO3 (s) ⇌ CaO (s) + CO2 (g) ∆H0 = 175 kJ We have to find how the amount…

13. For the decomposition of calcium carbonate CaCO3 (s) = CaO (s) + CO2 (g) ΔΗ175 kJ How will the amount (not concentration) of CaCO; (s) change with the following stresses to the system at equilibrium? a. CO2 (g) is removed. b. Cao (s) is added. The temperature is raised. с. d. The volume of the container is decreased.

13. For the decomposition of calcium carbonate CaCO3 (s) = CaO (s) + CO2 (g) ΔΗ175 kJ How will the amount (not concentration) of CaCO; (s) change with the following stresses to the system at equilibrium? a. CO2 (g) is removed. b. Cao (s) is added. The temperature is raised. с. d. The volume of the container is decreased.

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

Given that Kp - 3.0 x 10 for the reaction: 2 CO(g) C(graphite) + CO2(g). what is the partial pressure of CO2(g) at equilibrium if initially 4.00 atm of CO(g) is in contact with graphite? MA. 0.0024.atm B. 0.0060 atm C.0.0048 atm D.0.0012 atm E. 0.0096 atm
Consider the following reaction and its equilibrium constant: 12(g) 2 I(g) Kp = 0.209 A reaction mixture contains 0.89 atm 12 and 1.88 atm I. Which of the following statements is TRUE concerning this system? OA. The reaction quotient will decrease. OB. The reaction will shift in the direction of reactants. OC. The system is at equilibrium. D. The reaction will shift in the direction of products. OE. The equilibrium constant will decrease.
■ W Chapter... G N. O LCG a Ⓒ BA H H The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if K, and Q are within 5% of each other.) (a) 2 NH3(g) = N₂(g) + 3 H₂(g) [NH3] = 0.485 M, [N₂]; = 0.160 M, [H₂] = 0.110 M, K = 18 What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. O It will not shift. (b) 2 NH3(9) N₂(g) + 3 H₂(g) What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. P (NH3) = 1.90 atm, P(N₂) = 11.65 atm, P(H₂) = 11.65 atm, K = 6.6x104 O To the right, i.e. the product-side. O It will not shift. (c) 2 SO 3(g) 2 SO₂(g) + O₂(9) What is the reaction quotient? webassign.net [SO3] = 1.65 M, [SO₂), = 1.65 M, [0₂], =…
Which reaction, when at equilibrium, would be unaffected by a change in pressure? A. N2(g) + O2 (g) = 2NO(g) B. 2CO(g) + O2 = 2CO2(g) C. COBr2(g) = CO(g) + Br2(g) D. N2O4(g) = 2NO2 (g)
The reaction mixture below contains 0.305 atm of H2, 0.060 atm of S2, and 0.420 atm of H2S. 2 H2S(g) 2 2 H2(g) + S2(g) Kp = 2.4x104 at a particular temperature. Based on the information provided, select the correct relationship. K; the reaction will proceed to form more S2(g). Q > K; the reaction will proceed to the left. O More experimental data are needed to answer a question of this type. Q = K; the reaction is at equilibrium and no change is expected.
11. PLease refer to the attached photo. THank youuu
Explain deeply
Answer the following questions
Consider the following endothermic reaction: 4 PCl5 (g) ⇋⇋ P4 (s) + 10 Cl2 (g) How will the amount of Cl2 be affected if the total pressure of the system is increased? Select one: a. The concentration of Cl2 will increase. b. The concentration of Cl2 will decrease. c. The amount of Cl2 will not change.
$ . A sample of solld ammonium chloride was placed in an evacuated chamber, and then heated causing it to decompose according to the following reaction: NH4CI(S) NH3(g) + HCl(g) In a particular experiment the pressure of NH3(g) in the container was found to be 2.9 atm. Calculate the value of K₂ for the decomposition of NH4CI(s) at this temperature. Kp = R F Submit Show Hints Submit Answer 888 F4 % 5 T G Retry Entire Group 9 more group attempts remaining F5 Cengage Learning Cengage Technical Support A 6 MacBook Air Y F6 H & 7 ◄◄ F7 U J * 00 8 ► 11 F8 1 6a K ►► F9 O ) O F10 P 4) Previous Next F11 + " Save and Exit