Can you please check if my answers are correct? Thank you in advance Suppose a s

Question

Can you please check if my answers are correct?
Thank you in advance



Suppose a student mixes 5.00 ml of 2.00x10^-3 M Fe(NO3)3 with 5.00ml of 2.00x10^-3 M KSCN. The student determines the [FeSCN^2+] atequilibrium to be 1.40x10^-4.
Fe^3+(aq) + SCN^-(aq) <=> FeSCN^2+(aq)


* Calculate the initial number of moles of Fe^3+ and SCN^-

ANS: 1.00x10^-5 moles of Fe^3+
1.00x10^-5 moles of SCN^-


* How many moles of FeSCN^2+ are present at equilibrium? What isthe volume of the equilibrium mixture?

ANS: 1.40x10^-6 moles of FeSCN^2+
10 mL


* How many moles of Fe^3+ and SCN^- are consumend to produce theFeSCN^2+?

ANS: 1.40x10^-6 moles of Fe^3+
1.40x10^-6 moles of SCN^-

Explanation / Answer

Yes, what you've done is right. Initial moles of Fe3+ = molarity * volume                                = 2 * 10-3 M * 0.005 L                                = 1 * 10-5 moles Initial moles of SCN- = 2 * 10-3 M * 0.005 L                                = 1 * 10-5 moles                                = 1 * 10-5 moles total volume after mixing = 5 + 5 = 10 mL Moles of FeSCN^2+ = 1.40x10^-4. * 0.01 L                                    =1.40 * 10-6 moles
Fe^3+(aq) + SCN^-(aq) <=> FeSCN^2+(aq)
Since 1 mole of reactants reacts to form 1 mole ofproducts, moles of reactants consumed = moles of product formed = 1.40 *10-6 moles of Fe^+3 and SCN^2-.

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