Predict the equilibrium concentration of IBr in the reaction described below (for which Kc =280 at the reaction temperature) by constructing an ICE table, writing an equilibriumexpression for Kc, and solving for the equilibrium concentration. Complete Parts 1-3before submitting your answer.NEXT >In a 3.0 L container at high temperature, 0.400 mol of IBr is allowed to reach equilibrium. Fill in the ICE tablewith the appropriate value for each involved species to determine the partial pressures of all reactants andproducts. Where applicable, use the x variables to represent any unknown change in concentration.Initial (M)Change (M)Equilibrium (M)0.400 + x00.400 + 2x112(g) + Br₂(g) = 2 IBr(g)1₂(g)0.4000.400 - x0.1330.400-2r2++X0.133 + xBr₂(g)+2x0.133 + 2x3-X0.133 - x2 IBr(g)RESET-2x0.133 - 2x

ICE table will help us to find out the Kc. Kc is the equilibrium constant fro concentration terms.

Answered: Initial (M) Change (M) Equilibrium (M)…

Science

Chemistry

Initial (M) Change (M) Equilibrium (M) 1₂(g) + Br₂(g) 14 2 IBr(g)

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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