The rate law expression for the reaction is Rate = k[MnO4-].
To determine the rate law expression for the reaction of iron (II) with permanganate in acidic solution, we analyze the given data.
Comparing Trial 1 and Trial 2, the concentration of H+ is doubled while the concentrations of Fe2+ and MnO4- remain the same, but the rate does not change significantly.
Therefore, H+ does not appear to affect the rate, suggesting zero order with respect to H+ ions.
Comparing Trial 1 and Trial 3, doubling the concentration of MnO4- doubles the rate, indicating first-order with respect to MnO4-.
From Trial 1 and Trial 4, increasing the concentration of Fe2+ by a factor of 3 changes the rate insignificantly, suggesting it is also not affecting the rate, or zero order with respect to Fe2+ ions.
Therefore, the rate law is Rate = k[MnO4-].
The probable question may be:
Use the data of the balanced chemical reaction, between iron (II) and permanganate in acidic solution, to answer the following questions (a-c):
5 Fe^{2+} (aq) + MnO_4^- (aq) + 8 H^+ (aq) → 5 Fe^{3+} (aq) + Mn^{2+} (aq) + 4 H_2O (l)
Trial [Fe^{2+}] [MnO_4^-] [H^+] rate
1 0.010 M 0.025 M 0.050 M 3.12x10^{-4} M/min
2 0.010 M 0.025 M 0.100 M 3.04x10^{-4} M/min
3 0.010 M 0.050 M 0.050 M 6.31x10^{-4} M/min
4 0.030 M 0.025 M 0.100 M 2.71x10^{-4} M/min
a. Determine the rate law expression of the reaction