Use the table of data show below to calculate the value of the rate constant k.

Question

Use the table of data show below to calculate the value of the rate constant k. The reaction is first order. The reaction 2NO(g) + Br2(g) 2NOBr (g) is second order with respect to NO and Order with respect to Br2. Which is the correct rare law reaction ? The correct units for the rate constant k in the rate law The rate law for the aqueous reaction By what factor will the rate increase if we double the concentrations of all the three reactants ? given rate data below for the reaction Products, what is rate law for this reaction ? When the concentration of a reactant was 0.100 M, the rate of the rate of the reaction was 8.42 times 10-6 Ms-1 when the concentration of the reactant of the reactant was doubled to 0.200 M, the rate increased to What is the reaction with respect to this reactant (the value of "X" in the law) to three signification figures?

Explanation / Answer

    2NaOH + H2so4 ---> Na2SO4 + 2H2O

15. a=initial concentration = 0.124 M

a-x = concentration after 10 sec = 0.102 M

K = 2.303/tlog(a/a-x)

   = (2.303/10)log(0.124/0.102)

   = 0.0195 s-1

16. b) Rate = k[NO]^2[Br2]

17. k = rate/[A]^2[B]

      = m^-2*s^-1

C) m^-2*s^-1

18. rate = k[H2SeO3][I-]^3[H+]^2

         = K(2)(2^3)(2^2)

         = K 64

ANSWER : C) 64

19. (0.2/0.1)^n = (8.42*10^-5/1.59*10^-5)

n = 2.40

order = 2.40

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