13) Consider the following equilibria: SO2(g) + 0.502(g) SO3(g) 2NO3(g) 2NO2(g) + O2(g) Calculate the equilibrium constant for the reaction SO2(g) + NO3(g) = SO3(g) + NO₂(g). K. = 2.3 x 10-7 K. = 14x 10³

13) Consider the following equilibria: SO2(g) + 0.502(g) SO3(g) 2NO3(g) 2NO2(g) + O2(g) Calculate the equilibrium constant for the reaction SO2(g) + NO3(g) = SO3(g) + NO₂(g). K. = 2.3 x 10-7 K. = 14x 10³

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

Use the References to access important values if needed for this question. Consider the reaction: C(s) + 1/20₂(g) → CO(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: C(s) + O2(g) CO₂(g) K₁ CO(g) + 1/2O₂(g) = CO2 (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K =
Consider the following equilibrium reaction: PBr5(g) + 1/2 O2(g) = POB13(g) + Br2(g) Kc = 5.6 x 102 at 512 K Calculate K. for the reaction 2 PBr5(g) + O2(g) = 2 POBR3(g) + 2 Br2(g) at the same temperature. 24 1.1 x 103 280 5.6 x 102 O None of these 3.2 x 105
Consider the equilibrium at 25 °C 2 SO3(g) <==> 2 SO2(g) + O2(g) Kc= 3.58 x10-3 Suppose that 0.15 mol SO3(g), 0.01 mol SO2(g), and 0.0075 mol O2(g) are placed into a 10.0 L flask at 25 °C. Which of the following statements is true? Q > Kcand will shift from right to left. Q < Kc and will shift from right to left. Q > Kcand will shift from left to right. Q = Kcand the system is at equilibrium. Q < Kc and will shift from left to right.
Consider the reaction: N₂O4 (9) — 2NO2 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: N₂(g) +202 (g) = N₂O4 (9) K₁ 1/2N₂(g) + O2(g) — NO2(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K=
19. Given the following reaction: NH.CI (s) S NH3 (g) + HCI (g) AH= +42.1 kcal Suppose the above substances in the reaction are at equilibrium at 600 K in volume V and at pressure P. State whether the partial pressure of NH3 (g) will have increased, decreased, or remained the same in order to the equilibrium to be reestablished following the disturbances of the original system. Note that some solid remains in the flask at all times. Provide a one to two sentence explanation (a) The temperature of the system is increased (b) The volume of the system is increased (c) A quantity of gaseous NH3 is added. (d) A small quantity if NH4C1 is added.
A closed 1.00 L system initially containing 0.00200 mol H₂ and 0.00500 mol 1₂ at a given temperature is allowed to reach equilibrium Analysis of the equilibrium mixture shows that the amount of HI present at equilibrium is 0.00371 mol. Calculate the Kc at this temperature for the reaction. State whether the equilibrium is product-favored or reactant- favored at this temperature. H₂(g) +1₂(g) 2H1(g) Kc 31: The equilibrium is product-favored. Kc 31: The equilibrium is reactant-favored. Kc 0.032; The equilibrium is reactant-favored. Kc - 0.032; The equilibrium is product-favored.
2) Based on the information below, determine the value of the unknown equilibrium constant, Kc. 2 NOCl (g) « 2 NO (g) + Cl2 (g)Kc = 2.4 x 10-7 1/3 Cl2 (g) + 2/3 NO (g) « 2/3 NOCl (g)Kc = ?
The equilibrium constant Kc for the reaction,I2(g) + Br2(g) <-----> 2 IBr(g) is 26 at 425 K. What is the value of Kc for the equilibrium,1/2 I2(g) + 1/2 Br2(g) <-----> IBr(g) at 425 K?