Experiment Initial Relative rate Initial concentration of concentration of reactant X reactant Y (mol dm-³) (mol dm-³) 1 0.1 0.01 4 2 0.1 0.03 4 3 0.05 0.01 1 Given that the actual initial rate recorded in experiment 3 is 2.5 x 10-³ mol dm-³ s-¹, calculate the value of the rate constant for the reaction under the conditions of the experiment.

The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + H2- →I2 + 2 HCI Experiment [ICI],, M [H2]o, M Initial Rate, M s-1 1 0.339 7.80x10-2 |3.63х10-3 0.678 7.80x10-2 7.26x10-3 3 0.339 0.156 1.45x10-2 14 0.678 0.156 2.90x10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-2s-1.

At a certain temperature, initial rate data for the decomposition of gaseous N2O5N2O5 are as follows:   Experiment Initial [N2O5][N2O5] Initial Rate ofDecompositionof N2O5N2O5 (M/s)(M/s) 1 0.014 2.4×10−52.4×10−5 2 0.040 6.8×10−56.8×10−5 3 0.065 1.1×10−41.1×10−4   What is the value of the rate constant, including the proper units? Express your answer to two significant figures and include the appropriate units What is the initial rate of decomposition of N2O5N2O5 when its initial concentration is 2.0×10−2 MM ? Express your answer to two significant figures and include the appropriate units.

For the rate expression below, determine the exponents x and y for the following data. Rate = k [A] [B]Y Trial [A] M 1 2 3 4 0.10 Hint 0.20 0.10 0.30 x=1, y=0 x=0, y=1 Ox=1, y=2 x= 1, y=1 x=2, y=1 [B] M 0.20 0.20 0.10 Initial rate 4.6x10-2 9.2x10-² 2.3x10-2 0.30 1.4x10-1

The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.105 9.37×10-3 2 0.876 0.105 1.87×10-2 3 0.438 0.209 3.71×10-2 4 0.876 0.209 7.42×10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = _______    From these data, the rate constant is __________M-2s-1.

Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1 0.260 0.280 0.0119 A + B → C+ D 2 0.260 0.784 0.0933 3 0.312 0.280 0.0143 Units k = M-²s-1 M-'s-! M-s-!

Given that the rate constant for the decomposition of hypothetical compound XX from part A is 1.60 M−1⋅min−1�−1⋅min−1, calculate the concentration of XX after 13.0 minmin .

Find the overall order of the reaction, the rate constant, and the overall rate expression for the following set of experiments by using the kinetics method of initial rates. [A] 0.174 M [B] 0.968 M Expt volume A volume volume В time H20 (minutes:seconds) 19.083 mL 1 667 uL 250 uL 2:45 19.417 mL 333 uL 250 uL 5:26 3 667 uL 500 uL 18.883 mL 0:40

The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H Iz + 2 HCI Initial Rate, Ms! 1.57x10-2 3.13×10-2 6.24x10-2 0.125 Experiment [ICI]. M H), M 1 0.207 0.211 2 0.414 0.211 3 0.207 0.421 4 0.414 0.421 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is