A student fepeated the experiment mixed the following reactants: $2\mathrm{.}0mL$ of $4\mathrm{.}0M$ acetone, $1\mathrm{.}0mL$ of $1\mathrm{.}0MHCl,1\mathrm{.}0mL$ of $0\mathrm{.}0050M{l}_2$ and $1\mathrm{.}0mLH{H}_2.$

a$.$ By using the dillution equation $)=(M_2{V}_2$ calculate the concentrations of each reactant in the mixture after all of the solutions have been combined:

$[$acetone

$H^{+}$

b$.$ b$.$ Assuming the reaction took $145$ seconds, calculate the rate of the reaction $\frac{I_2}{}t.$

Rate of Reaction $=\frac{h_2}{4}=$

Using the answers above for the rate of the reaction and the diluted concentration of acetone, determine the order of the reaction with respect to acetone. $($called $x$ in the lab$)$

$($Use the logentinm method and calculare the value of $x$ io two decimal places and then round to the nearest integer.$)$

$x=,(2$ decimal places$)x=,(nearest$ integer$)$

Consider the following reaction $A+B$ products. The rate law was found to be

rate $=k[A{]}^2[B{]}^2$

a$.$ What is the order with respect to $A?$

b$.$ What is the order with respect to $B?$

c$.$ What is the overall order of the reaction?

d$.$ If the concentration of $A$ is doubled while the concentration of $B$ is kept constant, how will this affect the rate of the reaction?

e$.$ If the concentration of $B$ is doubled while the concentration of $A$ is kept constant, how will this affect the rate of the reaction?

If the concentration of $B$ is doubled while the concentration of $A$ is halved, how will this affect the rate of the reaction?

What safety precautions should you take during the experiment?