12. Which balanced chemical equation corresponds to the following equilibri,constant expression?KpPo PBr2A) 2 NOB (g) = 2 NO (g) + Br2(g)B) NO (g) + ½ Br2 (g) = NOBr (g)C) 2 NO (g) + Br2 (g) = NOBrD) 2 NO (g) + Br2 (g) = 2 NOBR13. You know that Kc = 2.0 at a certain temperature for the gaseous reactionA + 2B = C + 4D.What would be the value of Kc for the reaction2C + 8D = 2A + 4BA) 2.0B) 0.50C) 0.25D) 4.0 10. Sulfur trioxide decomposes according to the reaction:2 SO3 (g) = 2 SO2 (g) + O2 (g)In an equilibrium mixture at 1000 K you measure [SO3] =0.41 M, [S02] = 0.032 M,and the [O2] = 0.59 M. What is the value of Kc for this reaction at thistemperature?A) 3.6 X 103B) 1.1 X 101C) 2.2 X 10?D) 4.6 X 10411. At a certain temperature, the following reaction has a Kc value of 4.0 X 104:N2 (g) + O2 (g) = 2 NO (g)At equilibrium, you find [N2] = 0.25 M and the [O2] = 0.33 M. What is the [NO]?A) 6.8 X 103B) 5.7 X 103C) 1.7 X 105D) 3.3 X 105

Answered: Image /qna-images/answer/f967dee0-1976-4dca-83a0-23defc143344.jpg

constant expression? PROBr Kp = Po PBr2 A) 2 NOB (g) = 2 NO (g) + Br2(g) B) NO (g) + ½ Br2 (g) = NOB (g) %3D C) 2 NO (g) + Br2 (g) = NOB %3D D) 2 NO (g) + Br2 (g) = 2 NOB 13. You know that Kc = 2.0 at a certain temperature for the gaseous reaction A + 2B = C + 4D. What would be the value of Kc for the reaction 2C + 8D = 2A + 4B A) 2.0 B) 0.50 C) 0.25 D) 4.0

constant expression? PROBr Kp = Po PBr2 A) 2 NOB (g) = 2 NO (g) + Br2(g) B) NO (g) + ½ Br2 (g) = NOB (g) %3D C) 2 NO (g) + Br2 (g) = NOB %3D D) 2 NO (g) + Br2 (g) = 2 NOB 13. You know that Kc = 2.0 at a certain temperature for the gaseous reaction A + 2B = C + 4D. What would be the value of Kc for the reaction 2C + 8D = 2A + 4B A) 2.0 B) 0.50 C) 0.25 D) 4.0

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

What is the balanced equation for the following equilibrium expression? P3o, P'S02 Kp %3D Oa. 2s0 2(g) +0 2(g) 2SO 3(g) Ob. 2SO 3(g) = 280 2(g) + 0 2(g) Oc. SO 2(8).+0 2(g) = SO 3(g) Od. 2s0 2( aq) + O 2( aq) = 2SO 3( aq) O e. 2s0 3( aq) = 2SO 2( aq) + O 2( aq)
Use the References to access important values if needed for this question. Consider the following reaction where K. = 9.52x102 at 350 K. CH(g) + CC14(g) 2CH,C2(g) A reaction mixture was found to contain 2.21×102 moles of CH,(g), 3.87x102 moles of CC,(g) and 1.06×10 moles of CH,Cl,(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? d The reaction quotient, Qe, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium. Submit Answer Retry Entire Group 7 more group attempts remaining Previous Next 10:00 PM G O ) ENG 2/21/202 99+ 近

Ee.108.
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=
Consider the reaction: N₂O4 (9) 2NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: N2(g) + 202 (9) ⇒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
DUE NOW. Please answer it correctly by identifying the directions if forward or backward. Thank you!
Consider the following equilibrium:C2H6(g) + C5H12(g) <--> CH4(g) + C6H14(g); Kp = 9.57 at 500 KSuppose 45.4 g each of CH4, C2H6, C5H12, and C6H14 are placed in a 25.0-Lreaction vessel at 500 K. Which way will the reaction go? Why?
Given that Ka for HIO is 3.2 × 10-1" at 25 °C, what is the value of K, for IO¯ at 25 °C? Kp = Given that Kp for CH, NH, is 5.0 x 10-4 at 25 °C, what is the value of Ka for CH, NH; at 25 °C? Ka =
thank u in advance
Given the following equilibrium constants at 700K, 2 N2O(g) (double arrow) 2 N2 (g) + O2(g) K1 = 8.2 x 1033NO2(g) (double arrow) 1⁄2 N2(g) + O2(g) K2 = 2.44 x 108N2O4(g) (double arrow) 2 NO2(g) K3 = 4.6 x 10-3 determine the values of the equilibrium constants for the following reaction. Show your equation-buildingprocess and your calculations. 2 N2O4(g) (double arrow) 2 N2O(g) + 3 O2(g) K =
As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
Note: please use black ink and solve on a paper thanks