L. Using Le Châtelier's principle, predict the direction of equilibrium shift (to the left or right) in the following equilibria when the indicated stress is applied after the reaction has reached equilibrium. If no shift is expected, write "no change". A. PCI3(g) + Cl2(g) <----> PCI5(g) + energy; the reaction is cooled Select] B. CH4 (g) + 12 (g) <----> C2H412 (g) + heat; a catalyst is added Select] C. C2H6(g) + Cl2(g) <----> C2H5CI(s) + HCI(g); pressure is decreased Select) D. HPO42 (aq) + H2O(1) <----> PO4 (aq) + H30*(aq); NaOH is added Select] E. AgBr (s)<----> Ag* (aq) + Br" (aq); AgBr is added ( Select] F. CO (g) + 3H2 (g) <----> CH4 (g) + H20 (g); pressure is increased Select ]

L. Using Le Châtelier's principle, predict the direction of equilibrium shift (to the left or right) in the following equilibria when the indicated stress is applied after the reaction has reached equilibrium. If no shift is expected, write "no change". A. PCI3(g) + Cl2(g) <----> PCI5(g) + energy; the reaction is cooled Select] B. CH4 (g) + 12 (g) <----> C2H412 (g) + heat; a catalyst is added Select] C. C2H6(g) + Cl2(g) <----> C2H5CI(s) + HCI(g); pressure is decreased Select) D. HPO42 (aq) + H2O(1) <----> PO4 (aq) + H30(aq); NaOH is added Select] E. AgBr (s)<----> Ag (aq) + Br" (aq); AgBr is added ( Select] F. CO (g) + 3H2 (g) <----> CH4 (g) + H20 (g); pressure is increased Select ]

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

34.
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
12. A 2.50 L vessel contains 1.75 mole N₂, 1.75 mol H₂ and 0.346 mole NH3. What is the direction of reaction needed to attain equilibrium at 401 °C? The equilibrium constant Kc for the reaction is 0.50 at this temperature. N₂(g) + 3H₂(g) 2NH3(g)
The equilibrium constant for the following reaction is 0.18 at a set temperature. Find the equilibrium concentrations if the initial concentration of PCl3 is 0.225 mol/L and the initial concentration of Cl2 is 0.150 mol/L. PCI3(g)+CI2(g)=PCI5(g)
Consider the following equilibrium reaction: 2NO (g) + Cl2 (g) 2 NOCl (g) K=12 At equilibrium, [NOCl] = 1.60 M and [NO] = 0.80 M. The [Cl2] is
Consider the reaction. PCI, (g) = PCI, (g) + Cl,(g) K. = 0.0420 The concentrations of the products at equilibrium are [PC13] = 0.140 M and [Cl2] = 0.170 M. What is the concentration of the reactant, PCI5 , at equilibrium? [PC!5] = M
4. A. An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift"). a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.
Consider the following system at equilibrium at 600 K:COCl2(g) =CO(g) + Cl2(g)When some COCl2(g) is added to the equilibrium system at constant temperature: The reaction must: fill in the blank 1 A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CO will: fill in the blank 2 A. Increase. B. Decrease. C. Remain the same.
22) The ke for the equilibrium shown below is 45. Some methane and hydrogen sulfide are added to a container and at equilibrium the concentrations of methane and hydrogen sulfide are found to be 0.22 mol/L and 0.33 mol/L respectively. What are the equilibrium concentrations of carbon disulfide and hydrogen gas? CH4 + 2H2S(g) → CS2 (g) 4H2
5. The equilibrium constant expression of a gas reaction is [CS2] [H2]* _ [CH4] [H2S]? K. Write the balanced chemical equation corresponding to this expression
If this reaction is taking place in a 1.0L container, and 1.5 mol of SO2 were added to the reaction, whatwill the new concentrations of all fours gases be when equilibrium is reestablished?