SHOW WORK PLEASE SO I CAN DO THE REST OF MY HW BY LOOKING AT THIS QUESTION.
The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:
1. H2O2(aq) + I(aq) → H2O(l) + IO(aq) (slow)
2. IO(aq) + H2O2(aq) → H2O(l) + O2(g) + I(aq) (fast)
a. Assuming that the first step of the mechanism is rate determining, predict the rate expression for the overall process.
b. Write the chemical equation for the overall process.
you cant just not put the answer after finding it
a. To determine the rate expression for the overall process, we need to identify the rate-determining step (the slowest step in the mechanism). Given that the first step is considered to be the rate-determining step, we can use the stoichiometry of this step to write the rate expression.
From the first step of the mechanism, we see that for every one molecule of hydrogen peroxide (H2O2) reacting, one molecule of iodide ion (I) is consumed. Therefore, the rate expression for the first step is:
Rate1 = k1[H2O2][I]
Where k1 is the rate constant for the first step.
Since the first step is rate-determining, the overall rate of the reaction will be determined by the rate of the first step. Hence, the overall rate expression will be the same as the rate expression for the first step:
Rate overall = Rate1 = k1[H2O2][I]
b. The chemical equation for the overall process can be obtained by combining the two steps of the mechanism.
Step 1: H2O2(aq) + I(aq) → H2O(l) + IO(aq)
Step 2: IO(aq) + H2O2(aq) → H2O(l) + O2(g) + I(aq)
When we add these two equations together, the common species (H2O(l)) and (I(aq)) will cancel out, resulting in the overall chemical equation:
H2O2(aq) → H2O(l) + O2(g)
Therefore, the overall chemical equation is the decomposition of hydrogen peroxide to water and oxygen gas.
I've managed to find the answer for this question!
Thanks anyway!