t Using the Equilibrium Constant The reversible chemical reaction A B C +D has t
ID: 879724 • Letter: T
Question
t Using the Equilibrium Constant The reversible chemical reaction A B C +D has the following equilibrium constant CID 5.4 AlDB Part A Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units 0.7 M Submit Hints My Answers Give Up Review Part Incorrect, Try Again Part B What is the final concentration of D at equilibrium if the initial concentrations are Al- 1.00 Mand Bl 2.00 M? Express your answer to two significant figures and include the appropriate unitsExplanation / Answer
A + B <-----------------> C + D
2 2 0 0 -------------------> initial
2-x 2-x x x -----------------> equilibrium
Kc=[C][D]/[A][B]
5.4 = x^2 / (2-x)^2
2.32 = x / 2-x
4.65 - 2.32 x = x
4.65 = 3.32 x
x =1.4
equilibrim consentration of A = 2-x = 2-1.4 = 0.60 M
[A] = 0.60 M (two significant figures)
Part B )
A + B <-----------------> C + D
1 2 0 0 -------------------> initial
1-x 2-x x x -----------------> equilibrium
Kc=[C][D]/[A][B]
5.4 = x^2 / (2-x) (1-x)
5.4 = x^2 / 2-2x -x +x^2
5.4 x^2 -16.2 x +10.8 = x^2
4.4 x^2 - 16.2 x +10.8 =0
x = 0.87
equilibrium concentration of D = x = 0.87 M
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