Item 14 Part A At equilibrium, the concentrations of reactants and products can

Question

Item 14 Part A At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction 0.400 M·B $1.35 M . and C :0.450 M. The following A mixture initially contains A. B. and C in the following concentrations: A reaction occurs and equilibrium is established: A +2B C 0.600 M. Calculate the value of the equilibrium constant. Ke At equilibrium. A1-0.250 M and [C] Express your answer numerically. where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is Hints where [A, BC, and [D are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, ,instead of the equilibriunm constant, K Submit My Answers Give Up Part B where each concentration is measured at some arbitrary time t This question will be shown after you complete previous question(s) Continue

Explanation / Answer

A + 2 B <=> C
initially
0.400 . 1.35 .. .0.450
at equilibrium
-x . . . . .-2x . . . . .+x


[A]= 0.400 -x = 0.250
x = 0.150

[B] = 1.35 - ( 2 x 0.150)=1.05 M
[C]= 0.450 + 0.150 = 0.600 M

Kc = [C]/ [A][B]^2

= 0.600 / 0.250 ( 1.05)^2

= 0.600 / 0.250 *1.1025

=2.177

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