A flask is filled with 2.00 M CO₂, which decomposes according to the following reaction

2CO₂ (g) <-- --> 2CO (g) + O₂ (g)

Find the equilibrium constant of the reaction of the flask contains 0.90 M CO₂ at equilibrium.

The chemical reaction for the formation of the red-orange iron(III) thiocyanate complex ion is

Fe³⁺ (aq) + SCN^- (aq) <==> [FeSCN²⁺] (aq)

What is the source of the Fe³⁺ ions?

What is the source of the SCN^- ions?

The equilibrium constant for this reaction is given by

The stock solution in the stock beaker contains 10.00 mL of 0.1000 M iron(III) nitrate solution, 10.00 mL of 0.1000 M potassium thiocyanate solution, and 10.00 mL of 0.5000 M nitric acid solution.

What is the total volume of the stock solution? SHOW YOUR WORK!

How many moles of iron (III) nitrate are present in the stock solution? SHOW YOUR WORK!

How many moles of potassium thiocyanate are present in the stock solution? SHOW YOUR WORK!

Based on the moles of iron (III) nitrate and moles of potassium thiocyanate, how many moles of iron (III) thiocyanate do you expect to be formed (Hint: think limiting reagent)? We can do it this time because we have enough of one reagent to force the reaction to completion. SHOW YOUR WORK!

Once you determine the moles of iron (III) thiocyanate formed, determine the concentration of iron (III) thiocyanate in the final solution. SHOW YOUR WORK!