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. Notice that the iodide ion (I^-^) appears on both sides of the equations. This indicates that it is a spectator ion and does not undergo any change throughout the reaction. Therefore, we can cancel out the iodide ion, and the overall reaction will have the following form:
H2O2 → H2O + O2
The species that acts as a catalyst is indeed the iodide ion (I^-^), as it is present in both steps of the reaction but does not undergo any net change.
The reaction intermediate is a species that is formed during the reaction but is consumed again, without appearing in the final overall reaction. In this case, the reaction intermediate is OI^-^, which forms in the first step and is consumed in the second step.
Regarding the rate law for the overall reaction, it depends on the experimental data of the reaction rate. Without specific information, it is not possible to complete the rate law for the overall reaction accurately. The rate law is determined based on the concentrations of reactants, the order of the reaction with respect to each reactant, and the rate constant.