Assuming 1 mol of fe3+ and 2 mol of scn- were allowed to react and reach equilibrium. 0.5 mol of product was formed. the total volume at equilibrium was 1 l. how much fe3+ remained at equilibrium? (in mol) (1 point) your how much scn- remained at equilibrium? (in mol) (1 point) your what’s the equilibrium constant, kc? (1 point)

a. 0.5 mol

b. 1.5 mol

c. 0.67

Explanation:

Fe3+ + SCN- > [FeSCN]2+

a. The ratio of the product to Fe3+ is 1:1. Meaning that if 0.5 mol of product was produced up then 0.5 mol of Fe3+ was used. Leaving 0.5 mol remaining at equilibrium

b. The ratio of the product to SCN= is 1:1. Meaning that if 0.5 mol of product was produced up then 0.5 mol of SCN- was used. Leaving 1.5 mol remaining at equilibrium

c. KC =  0.5/(0.5*1.5) =  0.67

b.final