88.2k views
1 vote
Just need to know if I'm doing this right

Just need to know if I'm doing this right-example-1
User Robor
by
8.3k points

1 Answer

1 vote

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

User Puma
by
8.5k points

No related questions found

Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.