A reaction between substances A and B has been found to give the following data: 3A +2B 2C+D Al (mol/L) (mol/Rate of appearance of C 10 x 102 10 x 102 30 2.0 x 102 30 mol / L-hr) 0.300 x 100 810x 10 3 24 x 10-5 1.20 x 10-8 30 x 10-5 10 0 x 102 1.0 3.0 x 10- Using the above data, determine: a) the order of the reaction with respect to A and B - b) the rate law, and - c) calculate the specific rate constant

Be sure to answer all parts. For the following general reaction, rate -AJAJ and k-1.3 x 102 M.s. A+B 2C Use this information to fill in the missing table entries. Experiment JA] (M) BỊ (M) Initial rate (Mis) 1 0.013 0.250 2.20 x 10 2 0.026 0.250 3 0.500 2.20 x 10 1) Initial reaction rate in experiment 2: <10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3:

10. Which of the following reactions features the greatest kí/kĎ? kí is the reaction rate constant when all the hydrogen atoms in the organic reactant are 'H while kp is the reaction rate constant with all the hydrogen atoms in the organic reactant replaced by D (²H). OH OH to __ОН OH CI OH H₂SO4 heat HCI heat HCI heat Nal H₂SO4 heat CI CI

In the reaction                                                                                                                         C3H7Br(aq)  +  H2O(l) ---> C3H7OH(aq)  +  HBr (aq)  The concentration of the reactant changes from 0.0671 M at 125 seconds to 0.0549 M at 315 sec.  Calculate the average rate of decomposition.

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At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N205(8)→ 4NO2 (g) + O2(g) When the rate of formation of O2 is 3.6 x 10-3 M/s, the rate of decomposition of N2O5 is. M/s. A) 0.00090 OB) 1.4 x 10-2 1.8 × 10-3 OD) 3.6 × 10-3 E) 4.4 x 10-4

The data given in the table below is for the following reaction (run at 25°C): 2 NO + O, 2(g) → 2 (g) 2(g) Initial Concentration (M) Initial rate Experiment NO 0, Mol/(L · s) 1 0.0010 0.0010 7 x 10-6 2 0.0010 0.0020 14 x 106 3 0.0010 0.0030 21 x 10-6 4 0.0020 0.0030 84 x 10-6 5 0.0030 0.0030 189 x 106 1. Determine the orders of the reaction with respect to NO and O, (show all work): NO

[References] The reaction I (ag) + OCI (aq) → IO¯(aq) + Cl¯(aq) was studied, and the following data were obtained: I], (mol/L) [OCI"], (mol/L) Initial Rate (mol/L · s) 0.12 0.16 7.80 x 10-2 0.060 0.16 3.90 x 10-2 0.030 0.080 9.80 x 10-3 0.24 0.080 7.80 x 10- What is the rate law? (Use k for the rate constant.) Rate Calculate the value of the rate constant. k = L/mol · s Calculate the initial rate for an experiment where both I and OcI are initially present at 0.16 mol/L. Rate = mol/L · s

6. Given the reaction: CH3(CO)CH3 (M) | B(M) 0.010 0.010 CH3(CO)CH3 + I2 + H* → CH3(CO)CH2I + HI H* (M) Rate (M/s) 0.010 3.0 x 10-4 0.010 6.0 x 10-4 0.020 6.0 x 104 0.020 2.4 x 10-3 0.040 4.8 x 10-3 0.010 6.0 x 104 0.010 0.020 0.010 0.040 0.040 0.020 0.020 0.040 0.020 0.040 a. Determine the reaction order for each reactant. b. Solve for the rate constant, k, and the appropriate units. c. Write the rate law for the reaction, including a value for k. d. Solve for the rate of the reaction if there are 1.25 M of CH3(CO)CH3, 2.25 M of I2, and 3.25 M H*.

The reaction rate of CO and NO2 in the reaction   CO(g) + NO2(g) → CO2(g) + NO(g)   is measured using the initial rates method. The results are tabulated below. [CO] (mol/L)   NO2 (mol/L)   -([CO]/Δt (mol/L·s) 8.00 10-4   5.50 10-4   8.40 10-8 8.00 10-4   7.78 10-4   1.68 10-7 1.60 10-3   5.50 10-4   1.68 10-7             Determine the rate expression and calculate the rate constant for the reaction.