Step 1:H2O2 + I^-^ = H2O + OI^-^
step 2: H2O2 + OI^-^ = H2O + O2 + I^-^
What is the equation for the overall reaction? I am not sure how to do this since there are two equations.
Which species acts as a catalyst? I know that I^-^ is the catalsyt.
Which species acts as a reaction intermediate. I think it is O2
Complete the rate law for the overall reaction. I am not sure for this one.
To determine the overall reaction, you need to combine the two given equations by canceling out the common species on both sides of the equations. Let's analyze each species individually:
From the first equation:
H2O2 + I^-^ = H2O + OI^-^
From the second equation:
H2O2 + OI^-^ = H2O + O2 + I^-^
We can see that I^-^ appears on both the left and right sides of both equations. Thus, it is considered a spectator ion and can be canceled out. After canceling out I^-, the two equations become:
First equation (after canceling I^-^):
H2O2 = H2O + O
Second equation (after canceling I^-^):
H2O2 + O = H2O + O2
Now, if we combine the two equations, we get:
H2O2 + O = H2O + O2
This is the overall reaction equation.
Moving on to the species that acts as a catalyst. You are correct, I^-^ is the catalyst because it is present in the first step of the reaction but is regenerated and does not participate in the overall reaction.
The reaction intermediate is a species that is formed during the reaction but is consumed afterward. In this case, O2 is not considered an intermediate because it is one of the products. The reaction intermediate is generally a compound formed in one step and utilized/transformed in a following step. It appears in neither the reactant side nor the product side of the overall reaction equation. Therefore, there is no reaction intermediate in this case.
Regarding the rate law for the overall reaction, the rate law would be determined based on experimental observations. It is not possible to determine the rate law solely from the given balanced equations. The rate law describes how the rate of the reaction depends on the concentration of the reactants. It usually involves determining the order and rate constant for each reactant involved in the reaction. Without any additional information or experimental data, it is not possible to complete the rate law for the overall reaction equation.