Use the data in Table $1$ below to determine the reaction order for the decomposition of hydrogen peroxide $(H_2{O}_2),$ and calculate the value of the rate constant at the temperature of the experiment that produced the data.

Hydrogen peroxide $(H_2{O}_2)$ decomposes into water and oxygen with this reaction:

$H_2{O}_2(l)H_{2}O(l)+\frac{1}{2}{O}_2(g)$

Determine the reaction order of the decomposition of $H_2{O}_2$ by plotting the data $($Excel$)$ in three different ways. Fill out the table below to get all the numbers or have Excel calculate them for you. The graph with the largest $R^2$ value $($coefficient of correlation$)$ is the best fit for the data and gives us the correct reaction order for this reaction. Paste a copy of each graph into your upload or submit them along with your upload. $(5$ pts$)$ Note: $H_2{O}_2$ denotes Molarity of $H_2{O}_2.$

a$.$ time $($s$)$ vs$.[H_2{O}_2],$ zero order

b$.$ time $($s$)$ vs$.ln[H_2{O}_2],$ first order

c$.$ time $($s$)$ vs$.\frac{1}{H_2{O}_2},$ second order

$\backslash$table$[[$Time $($s$),[H_2{O}_2](M),ln[H_2{O}_2],\frac{1}{H_2{O}_2}$