Figure A. Rate of the reaction with increasing DER concentration while BLOOD and BEN concentrations are constant. 1. What is the order of reaction with respect to DER? 2. Calculate for the concentration of BLOOD after mixing for Runs 2 (x) and 3 (y). Run 2: Run 3: 3. Determine the order of the reaction with respect to BLOOD. Round off the answer to the nearest whole number.

Comment how the temperature affects the rate. a. Temperature definitely has an affect on the rate. When there is an increase in temperature, the rate at which the reaction occurs also increases. This is proved through my data. As each experiment had an increasing temperature, here are my rates that go from lowest to highest temperature: 3.25*10 M/s, 4.15*10 M/s, 6.85*10 M/s, 9.17*10* M/s. With this increase in temperature, there is therefore an increase in the energy of molecules in the solution. With this increase in energy, there is an increase in collisions with enough energy, and this ultimately leads to the rate increasing.

6. Reconsider the plot shown in Prelab Question 1. This plot shows a first order decay with an initial concentration of 0.010 M. Reaction Rate 0.0100 0.0080 0.0060 0.0040 0.0020 -0.0000 10 20 30 50 Time (s) a. Estimate the rate constant. b. Use your rate constant and equation 6 to estimate the half-life from the rate constant. c. Estimated the half-life directly from the plot. Are your two estimates of the half-life consistent? Explain why or why not. Concentration (M)

a. What is the overall order of the reaction? b. Write the rate expression. c. Calculate the rate constant, k. d. If the concentration of MnO4-, H2C2O4, & H+ are 0.155 M, 0.293M, and 0.475M respectively, what is the rate of the reaction?