Eau bnum constant and concent- Calculating Equilibrium Constants previous 13 of

Question

Eau bnum constant and concent- Calculating Equilibrium Constants previous 13 of 32 next Calculating Equilibrium Constants Deriving concentrations from data In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K In part B however, you wil be given initial concentrations and only one equilbrium concentration. You must use this data to The equilibrium constant, K, of a reaction at a find all three equilibrium concentrations before you can apply the formula for K particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium. Part B For a gaseous reaction with the general form The following reaction was performed in a sealed vessel at 756 °C the Ke and Kp expressions are given by Initially, only H2 and In were present at concentrations of Hal 3.55M and Ial 2.55M The equilibrium concentration of I2 is 0.0600 M.What is the equilibrium constant, Ker for the reaction at this temperature? Express your answer numerically. P (PA) (Pa) The subscript c or p indicates whether Kis expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be in the reaction, Submit Hints My Answers Give Up Review Part incorrect. Try Again; 9 attempts remaining Feedback Contnue

Explanation / Answer

Part B

H2 + I2 <==> 2HI

According to given problem [I2]eqm = 0.06 M

2.55-x = 0.06

or, x = 2.49 M

[H2] eqm = 3.55-2.49 = 1.06 M

[HI] = 2*2.49 = 4.98 M

Kc = [HI]^2/[H2][I2] = (4.98)^2/(1.06) (0.06) = 389.9

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Part A:

Kc = [CH3OH]/ [CO][H2] ^2

    =0.190 M/ (0.110)(0.140) ^2 = 88.13

H2 I2 2HI initial 3.55 2.55 0 change -x -x +2x equilibrium 3.55-x 2.55-x +2x

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