Question

5. The reaction of peroxydisulfate ion (S₂O₈²⁻) with iodide ion (I⁻) is

S2O82−(aq) + 3I−(aq) → 2SO42−(aq) + I3−(aq)

From the following data collected at a certain temperature, determine the rate law and calculate the rate constant.

Experiment	[S2O82−](M) .	[I−](M) .	Initial Rate [M/s]
1	0.0300	0.0840	8.80 × 10−4
2	0.0300	0.0420	4.40 × 10−4
3	0.0600	0.0420	8.80 × 10−4

(a) Which of the following equations represents the rate law for this reaction?

What is the rate constant for the reaction?

k = ______lmxs

6. From the data in the table, obtained at 360 K,

(a) determine the overall order of the reaction

Initial Rate of Disappearance of X (M/s)    [X] (M) [Y](M) 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30

(b) determine the initial rate of disappearance of X when the concentration of

X is 0.50 M and that of Y is 0.30 M.

_________ M/s

Answer 1

15. Let the rate law of the reaction is - rate = K[S208=1"[1]”...O Now, ist esfueriment; 8.80 x104=k 00.03)M (0.0842 2n0 29 : 4.407104 = *(0.03)M (0.042) 3rd 19 8.80 x 10 = 0.06) C0.042).. ② + gives => 8.80x10h 10.0845h es 2n=2=2" 8.80x104 (0.06 m. 6 + gives, 4+ 40 4164 = Bioso) or2 = 2 = 2 Putting the values of m & in into eqr ③ we get S. 80 109 = KX 0.03 0.084 ork - 8.80 x 10 9 8.349 0.03 x 0.084 = 0 - 349 ① we get the rate.se putting the values of min and k into ear low as → rate = 0.349 [S2085][1] K = 0: 349 Lmot' 51