I completed a lab to find the determination of Kc. I have to find the concentrations of reactants at equilibrium using an ICE table. The equation that were are using is
Fe^3+(aq) + SCN^-(aq) -> Fe(SCN)^2+(aq)
I have to create 5 ICE tables because we used 5 different test tubes each with a different concentration of SCN. The values I already have so far are the initial concentrations of reactants and the concentration of products at equilibrium.
For the first table the initial value of Fe is 1.0M and SCN is 1.0M. The concentration of product at equilibrium is 5.7 X 1o^-5M.
I set up the first ICE table like this:
Equation: Fe^3+ SCN^- Fe(SCN)^2+
I 1.0M 1.0M 0
C -5.7e-5M -5.7e^-5 +5.7e^-5
E 0.99M 0.99M 5.7e^-5
So for the concentrations of reactants at equilibrium, Fe is 0.99M and SCN is 0.99M
I put it in my calculator as 1.0 - 5.7 X e-5 and got 0.999943. So besides the weird number I got I'm guessing that I set it up correctly???
The last step is to determine Kc.
so it would be FeSCN / [Fe][SCN]
Kc= 5.7e-5M / (0.99m)(0.99M) = 5.8e-5
Did I set this up correctly??
Thank you for your help!!!
I think I know where I made a mistake.
For the initial concentrations of reactants Fe and SCN it says that I can use the table that was provided to determine how much the total volume of each solution was used.
The table that was provided provided the amount of Fe and SCN used in each test tube in mL.
So for test tube 1 it was 1.0mL of 0.005M Fe(NO3)3 and 1.0mL of 0.005M KSCN
For all 6 of the test tubes used 1.0mL of Fe was used. Do I need to use the c1v1=c2v2 equation or is the initial concentration for Fe 0.005M?
Test tube 1 is
(Fe) = 0.005M x (1.0 mL Fe/2 mL total) =?
(SCN) - 0.005M x (1.0 mL SCN/2.0 mL total) = ?
Where did the 2mL come from?
Oh I see that's the total of SCN and Fe but we also used 0.1M HNO3 so for the first test time we used 5mL of HNO3 with the Fe, SCN so the total would be 7mL.
Fe= (0.005M) (1.0mL) = x(7mL) = 0.000714 So 7.1 e-4 Correct.
The teacher said to put the answer in 2 sig figs.
The Fe will be (?M at start x (mL Fe/total volume)
The SCN will be (?SCN at start x (mL Fe/total volume).
Right so for Fe I did (0.005M) (1.0mL Fe) / (7.0mL total of solutions in the tube) = 7.1e-4.
So then my ICE table would say 7.10e-4 for both Fe and SCN because SCN for tube 1 had the same amounts and then I would subtract 7.1e-4 by the concentration of product which was 5.7e-5. This would be 6.53e-4M for concentration of reactants for Fe and SCN correct?
Yes, you have set up the ICE table correctly for the given reaction. The initial concentrations of Fe^3+ and SCN^- are both 1.0M, and the concentration of Fe(SCN)^2+ at equilibrium is 5.7e-5M.
In the ICE table, you correctly assign the initial concentrations of Fe^3+, SCN^-, and Fe(SCN)^2+ under the columns I (Initial), C (Change), and E (Equilibrium). Since the stoichiometry of the reaction is 1:1:1, the change in concentration for Fe(SCN)^2+ is equal to the equilibrium concentration. Therefore, you correctly put 0 under the Change column for Fe(SCN)^2+.
For the concentrations of reactants at equilibrium, you correctly calculate that Fe^3+ is 0.99M and SCN^- is 0.99M by subtracting the equilibrium concentration of Fe(SCN)^2+ from the initial concentration of Fe^3+ and SCN^-.
However, when calculating the concentration of Fe^3+ at equilibrium, your calculation of 1.0 - 5.7e-5 gives you the value of 0.999943, not 0.99. This appears to be a calculator error or a typographical error in your submission. The correct calculation should yield 0.99.
Lastly, when calculating Kc, you correctly write the expression Fe(SCN) / [Fe][SCN] and substitute the given values to obtain Kc = 5.7e-5M / (0.99M)(0.99M) = 5.8e-5. So, overall, you have set up and solved the problem correctly.
Please double-check your calculations for the concentrations of reactants at equilibrium to ensure the correct values are used in further calculations.