Answered: For the following reaction, the Kc is…

For the following reaction, the Kc is 1.89 at 933K. H2(g) + CO2(g) H2O(g) + CO(g) Calculate the equilibrium concentration of hydrogen, [H2], when [CO2] = 0.210M, [H2O] = 0.390M, and [CO] = 0.160M.

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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Given the reaction: CO(NH2),(s) + H2O(g) = CO2(9) + 2NH3(g) -- Kp If this reaction system is initially at equilibrium and a catalyst is added, the new position of equilibrium will be = 1.39 at 500 K The value of K, for the given reaction at 600 K is The reaction CO(NH₂)₂(s) + H₂O(g) → CO₂(g) + 2 NH₂(g) is -- A flask containing CO₂(g), NH₂(g), CO(NH₂)₂(s) and H₂O(g) is initially at equilibrium at 500 K. When the flask is heated to 600 K, the amounts of CO(NH₂)₂(s) and H₂O(g) decrease and the amounts of CO₂(g) and NH₂(g) increase. This means that:
35 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 3.01 × 10³ at 900 K. If an initial mixture of 0.0216 mol SO2 and 0.0148 mol O2 reacts in a 1.0 L vessel, what will be the concentration of SO3 at equilibrium? 2 SO:(g) + O2(g)= 2 SO:(g) 1 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. 2 SO:(g) O:(g) + 2 SO:(g) Initial (M) 0.0216 0.0148 Change (M) 0.0216 - 2x 0.0148 - x Equilibrium (M) 5 RESET 0.0216 0.0148 1.0 +x +2x -2x 0.0216 + x 0.0216 + 2x 0.0216 - x 0.0216 - 2x 0.0148 + x 0.0148 + 2x 0.0148 - x 0.0148 - 2x
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: so,(9) + 1/2 02(9)so3(9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K1 and K2, for the reactions below: 2 S(s) + 3 02(9)=2 s03(g) K, S(s) + 0,(9) so,(9) Ka For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared.
Chemistry
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= [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH₂Cl2 (9) CH4 (9) + CCl4 (9) = Calculate the equilibrium concentrations of reactant and products when 0.315 moles of CH₂Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂Cl₂] = [CH4] [CC14] = = Submit Answer Show Hint NOV 30 Q F4 M M M Retry Entire Group 9 F5 + tv ♫ 8 9 more group attempts remaining MacBook Air C F6 < F7 DII F8 Previous Email Instructor F9 O Next Save and Exit J F10
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