The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc = [C][D] / [A][B] =7.0?
Initially, only A and B are present, each at 2.00M. What is the final concentration of
A once equilibrium is reached?
What is the final concentration of D
at equilibrium if the initial concentrations are [A]= 1.00M [B]= 2.00M?
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Hypothetical equilibria......
A ....+..... B <====> C + D ............ Kc = 7.0
2.00M ... 2.00M ....... 0 .. 0 ............ Initial
-x ........... -x ........... +x ..+x ........... Change
2.00-x.....2.00-x ....... x... x............. Equilibrium
Kc = [C][D] / [A][B]
7.0 = x² / (2.0-x)²
--- some algebra goes here ---
x = 1.45
[A] = 0.55M
==========
A ....+..... B <====> C + D ............ Kc = 7.0
1.00M ... 2.00M ....... 0 .. 0 ............ Initial
-x ........... -x ........... +x ..+x ........... Change
1.00-x.....2.00-x ....... x... x............. Equilibrium
Kc = [C][D] / [A][B]
7.0 = x² / [(1.0-x)(2.0-x)]
--- some algebra goes here ---
x = 0.90
[D] = 0.90M