5. Studying the Temperature Dependence of the Rate Constant (k). The following reaction is studied at 3 different temperatures. Below you will find the rate constant for a reaction determined at these temperatures. Use this data to answer the following questions A–>B k (min-') 0.0409 min 0.0818 min-! 0.157 min T (Celsius) 25.0 °C 35.0 °C 45.0 °C (a) Calculate In k and 1/T and provide the values in the table below. In k 1/T (K') (b) Plot In k vs. 1/T and attach the graph. It should be linear. (c) Calculate the slope of the graph of In k vs. 1/T. Show your work below.

Q1. Which of the following reactions will be the fastest to be complete? Q2. Discuss each factors that will affect the rate of reaction to receive full points. Factors Reaction #1 Reaction #2 Reaction #3 Reactant 5 M 5 M 5 M Concentration Surface Area Small Large Large Temperature 25 °C 35 °C 20 °C Catalysts Yes Yes No

4. Determine the order of the following reactions from the rate constant. a. k= 1.3 x 104 s-1 b. k = 4.7 x 10-² mol L-'s'

Consider the following balanced chemical reaction: A + B → C The following table shows initial reaction rates obtained using different initial concentration of A and B: Initial [A] (mol L-) Initial [B] (mol L-1) Initial Rate (mol L-1 s-1) 0.202 0.350 0.138 0.202 0.701 0.277 0.604 0.350 0.413 0.604 0.701 0.827 If rate = k[A]"[B]" , then m = • and n =

Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) SO₂(g) + Cl₂(g) [SO₂Cl₂], (M) k= 0.100 0.200 0.300 Initial rate (M/s) 2.00 x 10-6 4.00 x 10-6 6.00 x 10-6 Determine the value and units of the rate constant. units:

3. The following mechanism is proposed for the reaction of chlorine with chloroform: Cl, + CHCI, CCI, + HCI Cl, Step 1 fast equilibrium 2Cl CHCI, +CI » HCI +CCI, CCI, +Cl»cCI, Step 2 slow Step 3 fast a) Show that this mechanism gives the correct, overall balanced reaction equation. b) Write the rate law predicted by this mechanism.

Subject-advance chemistry

Using the reaction and data in the table below answer the following series of questions.   Reaction NO conc. O2 conc. Initial Rate (M/s) 1 0.500 M 0.200 M 2.2 x 10-4  2 0.250 M 0.200 M 5.6 x 10-5 3 0.250 M 0.400 M 1.1 x 10-4 *conc = concentration a.  The reaction is                             order in regards to NO. b.  The reaction is                               order in regards to O2.