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Would this be correct?
Consider the following two reactions:
5 Fe2+(aq) + MnO41-(aq) + 8 H1+(aq) = 5 Fe3+(aq) + Mn2+(aq) + 4 H2 O(l)
2 MnO41-(aq) + 5 C2O42-(aq) + 16 H1+(aq) = 2 Mn2+(aq) + CO2 (g) + 8 H2 O(l)
Both of these reactions result in the purple permanganate (MnO41-(aq)) ion reacting to form the colourless manganese (II) ion. The difference is that the first reaction happens in a few seconds, while the second occurs over several minutes. Explain why this so, based on what you know of chemical reactions and what you can see in these two reaction equations.
The first reaction would have more concentration ( solvent would be able to dissolve in solute) and as stated above the chance of a collision happening increases so the number of collisions that result in a chemical reaction increases as well. As the number of effective collisions increases, the rate of reaction increases.
2 Answers
- ColinLv 78 years agoFavorite Answer
The big difference between the two depends on two factors.
1) the activation energy for the ethanedioate reaction (oxalate) is far higher than the Fe2+ reaction so initially it is much slower due to the slow rate of production of products. Hence the second reaction is normally heated to ensure more collisions to get it going.
2) as the reaction proceeds the rate becomes quicker for the second reaction as one of the products Mn2+ catalysed the reaction and hence lowers the activation energy causing rate to increase as time proceeds.
Source(s): Rtc
