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Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 55.6 at 698 K. H₂(g) + 12 (9)2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.254 moles of H₂ and 0.254 moles of I2 are introduced into a 1.00 L vessel at 698 K. M [H₂] [1₂] = [HI] = = Submit Answer M M Retry Entire Group 9 more group attempts remaining

Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 55.6 at 698 K. H₂(g) + 12 (9)2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.254 moles of H₂ and 0.254 moles of I2 are introduced into a 1.00 L vessel at 698 K. M [H₂] [1₂] = [HI] = = Submit Answer M M Retry Entire Group 9 more group attempts remaining

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Submit Answer [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 55.6 at 698 K. H₂(g) + 12 (9) → 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.254 moles of H₂ and 0.254 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H₂] = | M [1₂] = [HI] = M M Retry Entire Group bartleby 9 more group attempts remaining
Transcribed Image Text:Submit Answer [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 55.6 at 698 K. H₂(g) + 12 (9) → 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.254 moles of H₂ and 0.254 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H₂] = | M [1₂] = [HI] = M M Retry Entire Group bartleby 9 more group attempts remaining
Expert Solution
Step 1: Introduction to the givcen data

The chemical equilibrium is a state in which both reactants and products involved in reaction are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system.
The given reaction is the

H subscript 2 left parenthesis g right parenthesis space plus space I subscript 2 left parenthesis g right parenthesis rightwards harpoon over leftwards harpoon space 2 H I left parenthesis g right parenthesis comma space

equilibrium constant of the given reaction, Kc = 55.6

Given that the initial number of moles of H2 = 0.254 mol

The initial number of moles of I2 = 0.254 mol

The initial concentration of H2 = fraction numerator n u m b e r space o f space m o l e s over denominator v o l u m e space o f space t h e space s o l u t i o n space end fraction equals fraction numerator 0.254 space m o l over denominator 1.0 space L end fraction equals 0.254 space m o l divided by L space equals space 0.254 space M

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