the reaction is CO + SO3 <=> CO2 + SO2, the rate law for this reaction is rate=k[SO3] and the mechanism is
SO3 -> SO2 + O
CO + O -> CO2
Which is the slow step? I have to find catalysts and intermediates and is O both catalyst and intermediate? If it isn't, what is it?
To determine the slow step in the given reaction mechanism, we need to compare the rate-determining step (RDS) of each elementary step. The slowest step is the one that has the highest activation energy and determines the overall rate of the reaction.
The given mechanism consists of two elementary steps:
1. SO3 -> SO2 + O
2. CO + O -> CO2
To determine the slow step, we compare the reactive species involved in each step. In the first step, the reactive species are SO3 and O, while in the second step, the reactive species are CO and O. Since O is common to both steps, we can consider it as an intermediate rather than a catalyst.
Now, let's compare the concentration of the reactive species in each step. In the first step, the concentration of SO3 is involved in the rate equation, while in the second step, the concentration of CO is relevant.
Since the rate equation for the given reaction is rate = k[SO3], it indicates that the concentration of SO3 determines the reaction rate. Therefore, the slow step of this reaction mechanism is the first step: SO3 -> SO2 + O.
As for catalysts, a catalyst is a substance that speeds up a reaction by providing an alternative reaction pathway with lower activation energy. In the given mechanism, no catalyst is mentioned. Therefore, we don't have any catalysts in this particular reaction.
To summarize:
- The slow step in the mechanism is the first step: SO3 -> SO2 + O.
- O is an intermediate, not a catalyst.
- There are no catalysts mentioned in this reaction mechanism.