What is the final concentration of D at equilibrium if the initial concentration
ID: 951565 • Letter: W
Question
What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?The reversible chemical reaction
A+BC+D
has the following equilibrium constant:
Kc=[C][D][A][B]=5.3
Gaseous hydrogen iodide is placed in a closed container at 425C, where it partially decomposes to hydrogen and iodine:
2HI(g)H2(g)+I2(g)
At equilibrium it is found that [HI]= 3.55×103M, [H2]= 4.82×104M , and [I2]= 4.82×104M.
What is the value of Kc at this temperature?
b
The reversible chemical reaction
A+BC+D
has the following equilibrium constant:
Kc=[C][D][A][B]=5.3
a
Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached?
b
What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?
Explanation / Answer
A + B C + D
initially 1 2 0 0
at equi (1 - X) (2 - X) X X
Kc=[C] [D] / [A] [B] = 5.3 = (x) *(x) / ((1-x)*(2-x))
x = 0.8726 = [D]
2 HI (g) H2 (g) + I2 (g)
at equi 3.55×103 4.82×104 4.82×104
Kc = [HI]^2 / [H2] [I2]
Kc = (3.55 * 10^-3)^2 / (4.82*10^-4)^2
Kc = 54.2453
A + B C + D
initially 2 2 0 0
at equi (2- X) (2 - X) X X
Kc=[C] [D] / [A] [B] = 5.3 = (x) *(x) / ((2-x)*(2-x))
x = 1.3943 = [D]
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