We’re being asked to determine the equilibrium concentrationof C given the following equilibrium reaction:
2 A(aq) + B(aq) ⇌ 2 C(aq); Kc = 1.5x10-8
We know that the initial amount of A and B is 0.1 M. From this, we can construct an ICE table:
Kc is the equilibrium expression of the concentrations in the reaction. The general form of an equilibrium expression is:
The following reaction has a Kc at 520. K equal to 1.50 × 10–8:
2 A(aq) + B(aq) ⇌ 2 C(aq)
If the reaction is started with 0.100 M A and 0.100 M B, what is the equilibrium concentration of C?
A. 3.75 × 10–12 M
B. 1.94 × 10–6 M
C. 3.87 × 10–6 M
D. 7.50 × 10–12 M
E. 1.50 × 10–11 M
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