The expectation for this assignment is that each student will complete it individually and turn in their own original work: Use Collision Theory to explain why the following factors affect the rate of reaction: 1. Concentration 2. Temperature 3. Particle orientation Mercury (II) chloride reacts with the oxalate ion according to the following chemical equation: 2HgCl2(aq)+C2O42(aq)2Cl(aq)+2CO2(g)+Hg2Cl2(s) The reaction was carried out three times and the rate of the reaction was measured. The following table shows the concentrations of the reactants and the corresponding rates. The generic rate law for this reaction looks like this: rate =k[HgCl2]x[C2O42]y 8. Determine the value of the rate constant, k. Include the correct units. 9. At this point, you kinow the values of x,y, and k. Substitute the numerical values of x,y, and k into the rate law (include the units for k ): rate=[HgCl2][Cr2O42] 10. The rate law for the reaction of nitric oxide (NO) with oxygen (O2) is: rate=0.54M2s1[NO]2[O2](at300C) Calculate the rate of reaction if initial concentration of NO is 0.008M and the initial concentration of O2 is 0.005M