Plus minus Using the Equilibrium Constant The reversible chemical reaction A+ B

Question

Plus minus Using the Equilibrium Constant The reversible chemical reaction A+ B C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=4.9 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. [A] = Value Units Part B What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M Express your answer to two significant figures and include the appropriate units. [D] = Value Units

Explanation / Answer

a) let the final concentration of A be x.so

so [B]=x.

[C]=[D]=2-x

so,

Kc=(2-x)^2/x^2=4.9

or x=0.622 M

b) let the concentration of D be x.so,

[A]=1-x, [B]=2-x, [C]=x.so,

4.9=x^2/((1-x)*(2-x))

or x=0.865 M

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