Construct an \"I.C.E.\" table (Equilibrium table) to calculate the equilibrium c

Question

Construct an "I.C.E." table (Equilibrium table) to calculate the equilibrium concentrations of each species (Fe^3+, HSCN, FeSCN^2+, and H^+) in solution for each temperature. The "I" stands for the "Initial" concentrations, "C" stands for the "Change" in concentration that occurs as equilibrium is established, and "E" denotes the "Equilibrium" concentrations. Use the M_1 V_1 = M_2 V_2 relationship to determine the initial concentrations of each species added to the test tube. For example, in Test Tube solution 6 you added 5 mL (V_1) of the 0.00200 M Fe(NO_3)_3 solution (M_1) (0.00200 M Fe^3+). Each test tube has a total volume of 10 mL (V_2). The Fe^3+ concentration after all solutions are mixed (M_2) is: M_2 = [Fe^3+] = M_1 V_1/V_2 = (0.00200M)(5 mL)/(10 mL) = 0.00100 M Fe^3+ Calculate the initial concentrations of all the other species in a similar fashion with the exception of the HNO_3 concentration which is constant throughout, since all other solutions are made with 0.500 M HNO_3. Here is an example for Test Tube solution number 6: As the reaction proceeds, "x" moles of FeSCN^2+ are product from "x" moles of Fe^3+ and "x" moles of

Explanation / Answer

For the Calculated Values row, you need to fill the values for the corresponding columns.

For this you basically need the value of 'x', which is [FeSCN2+]. This is known from the previous table where you have calculated the equilibrium conc. using absorbance method.

But the values are all greater than 0.0002, which is not possible because x has to be less than 0.0002 else [HSCN] would become -ve.

Kindly correct the readings in the first table and then use the appropriate value for 'x'

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