What if the equation for the equilibrium were: Fe^3+ (aq) + 2SCN^- (aq) rightlef

Question

What if the equation for the equilibrium were: Fe^3+ (aq) + 2SCN^- (aq) rightleftharpoons Fe(SCN)_2 +(aq) How would the expression for the Ke be written? If the reaction in question 1 is correct, the concentrations of Fe3+ at equilibrium in each sample would be the same as you calculated in part 2 of the calculations section. But the values for the equilibrium concentrations of SCN- would change. They would be calculated as follows: [SCN-]_initial - 2[[Fe(SCN)_2^+] = [SCN^-]_eq. Why is that? (Assume that the spec 20 measurements still gave correct values for the concentration of the product.)

Explanation / Answer

That happens because not all SCN is converted to and there is a remaining amount in the sample.

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