A chemist would like to explore the reaction of compounds "A" and "B" to make "C", in order to determine the reaction stoichiometry and equilibrium constant.A reaction container is initially prepared with 0.1M of each reagent and will be allowed to come to equilibrium. The chemist has two hypotheses for how thereaction could proceed. Which outcome from the list below would match with each hypothesis?Initial Conditions:0. 150. 1250.10.0750.050.025A B1.0. 150125a. 156 1250.0750.05Equilibrium conditions ifreaction is:3.a. 150 125A +B cAnd the Kc = 2.5S 0.075o.05Equilibrium conditions ifreaction is:A +B 2CAnd the Kc - 2.54.S 0.0755.O 1250.10.0750.os0.025Concentration (M)Concentration (M)

Equilibrium refers to a situation in which the concentration of reacting species do not change over…

Answered: Equilibrium conditions if reaction is:…

Equilibrium conditions if reaction is: A+B=c And the Kc = 2.5 Equilibrium conditions if reaction is: A+B= 2C And the Kc = 2.5

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...

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Questions from Lab: Equilibrium and Le Chatelier's Principle 1.Consider the chemical reaction: N2+ 3H2 yields 2NH3. The equilibrium constant is K = 6.0 x 10-2, and concentrations are as follows [H2] = 2.5 x 10-1 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10-4 M. Is the reaction at equilibrium? If not, which direction would it shift? Show your calculations. 2. Given this reaction at equilibrium, C(s) + CO2(g) D 2CO(g) (∆H° = 119kJ), explain the changes that would occur when the following stresses are applied: a.CO is removed. b.Heat is removed. c.CO2 is added.
4. The reaction X + Y 2 Z is one that essentially goes to completion at equilibrium. Which of the following values is most likely the Kc for this reaction? a) 2.6 x 10-18 b) 3.5 x 10-2 c) 1.00 d) 4.7 x 105 e) 1.06 x 10-14
1) 4.5 x 104 M. The initial concentration of B is 5.3 x 103 M. At equilibrium, the concentration of A is 1.2 x 104 M. What is the value of Keg? All of the reagents in the reaction below are in aqueous form. The initial concentration of A is A + 2B C + 3 D
On the basis of Kc for the following reaction, would you expect the reaction to go almost completely to product at equilibrium? N2(g) + 2O2(g) ↔ 2NO(g); Kc = 3x10-17 yes or no
At 475 oC, Keq = 0.230 for the reaction: 1/3 NO2(g) + 1/3 N2O(g) (equilibrium arrows) NO(g) (a) What is the value of Keq for the reaction NO(g) 1/3 NO2(g) + 1/3 N2O(g)?Keq = .(b) What is the value of Keq for the reaction NO2(g) + N2O(g) 3 NO(g)?Keq = .(c) What is the value of Keq for the reaction 3 NO(g) NO2(g) + N2O(g)?Keq = .
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answer #9
Given the following equilibrium constants at 415°C, Naz 0(s) 2 Na(1)+02(9) K1 = 9 x 10-25 Na0(g) Na(1) + 02 (9) K2 = 2 x 10-5 NazO2(s) 2 Na(1) + O2 (g) NaO2 (s) = Na(1)+02(g) K3 = 5 x 10-29 KA = 8 x 10 14 determine the values for the equilibrium constants for the following reactions: a. Naz 0(s) +02 (g) Naz O2 (s) Equilibrium constant b. NaO(g) + Naz 0(s) Naz O2 (s) + Na(l) Equilibrium constant = c. 2 Na0(g) - Naz O2 (s) Equilibrium constant = (Hint: When reaction equations are added, the equilibrium expressions are multiplied.)
(Q97) What is the value of the equilibrium constant (Keg) for the following hypothetical reaction: 2 W (g) + X (g) 3 Y (g) Using the related hypothetical equations should be helpful: X (g) + 1/2 Y (g) W (g) + 1/2 Z (g). K1 = 0.316 %3D 2 Y+Z 3 X (g) K2 = 118
7 4 (a) Calculate the value of Kc for the reaction: PC15 (2) PC13 (g) + Cl2 (g) AH = Positive Given that when 8.4 mol of PCls (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PCls (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (1) Increasing temperature (ii) Lowering the concentration of chlorine (Cl2) (iii) Addition of a catalyst
Equilibrium Constant 82 4) ½N2(g) + 02(g)= NO2(g) Kc 1.04 x 10-9 N2(g) + 202(g) N204(g) Kc =7.42 x 10-18 %3D Calculate Kc for each of the following. (a) 2NO2(g) = N2(g) + 202(g) (b) N2(g) + 202(g) = N2O4(g) PA at O002 16 mnundiliupo 0002 10 eft 00. Cci boouho ss sllo eolom 02.1 bae chHto estom 021 H Tondiliupe is inso H lo esfomem won (c) 2NO2(g) = N2O4(g) a li nao adt ai ol borsluoleg uor asulev od of qued blooerW ( ort nadw M000,0 bau o oldeid 2aw bo ov suiev ol enos walha g0)dgid 2aw bo oy eulev TUwens uoy nislg M00.210 oulsDsd in la6