Let's go over how to determine the rate law for the reaction In this problem, we need to find the experiments in which one of the reacting concentrations remains the same and one of them changes. So if we look at reaction one and three, we can see that hydrogen peroxide concentration remains the same and the iodide concentration changes. So let's take a look at how the iodide concentration changes and how this changes the eight of the reaction. So if we divide the concentrations of iodide, then we see that the concentration goes up by a factor of four. Now we're going to do the same with the rates. So we're going to take The rate from reaction three. The boy by The rate from reaction one. We also get about four. So from this we can see since the concentration and the reaction rate go up by the same factor. This reaction is first order in the aisle diet ion. Now, we're going to look at experiment two and four. So in these two experiments, you can see that the iodide ion concentration say the same, but the hydrogen peroxide concentration is changing. So let's determine how the hydrogen peroxide concentration changes. So if we divide the concentrations, We see that the concentration goes up by a factor of two, and they were going to do the same for the rates. And we see that is also a factor of two. So, because the concentration and the rate is going up by the same factor, it's also a first order in hydrogen peroxide. So this is going to be the expression for the Great Law. Now we are asked to calculate the value of K. To get the value of K. We're going to plug in the numbers from any experiments. So, I'm just going to do experiment one. So now we're going to plug in the numbers Mhm. And now, So for cake. So this is the value that we get for K. Now we're giving some reaction conditions and we add K I. As well as a solution of hydrogen peroxide. In this case, one more of KI contributes one more of the I have died ion. So since we know this, if we calculate the moles of K I, we have also calculated the moles of iodide ion. So what we're going to do is we're going to take the mole aren t of the solution, multiply it by the volume, which we need to convert two leaders first And then we're going to put that over the total volume. And we're told that we have 25 ml at its 25 million. So the total volume is 50 Bill leaders. Then this will give us the polarity of the iodide ion. So now we have to determine the modularity of the hydrogen peroxide. So we're going to use the density and the volume to find the mass. The density is one g over one millimeter And we have 25 ml of the solution. So that means that we have 25 g of the solution. 10% of this is a hydrogen peroxide. So we're going to convert the percentage to a decimal, multiply it by the mass of the solution and that will give us a massive hydrogen peroxide. Now that we have the mass of the hydrogen peroxide, we can convert two moles of hydrogen peroxide using the molar mass. So from a periodic table we get the molar mass. Well the masses 34.01 g. And that loves to convert two moles. And then we're going to put this over the total volume, which is as many leaders. And then we're going to end up with the polarity of ha jin peroxide. Now that we have the more clarity of both of the reactant. We are going to solve for the rate using the rate law. So we calculated the value of K earlier and we can use that. And we're just going to plug in the numbers and recall that this reaction is first order in both the iodide ion and the hydrogen peroxide. So then we're just going to multiply everything together. So we get .36 polarity per minute as the rate.