Consider this reaction and the experimental quantities given in the table. 9I -
ID: 853287 • Letter: C
Question
Consider this reaction and the experimental quantities given in the table.
9I- + ClO3- + 6H+ -> 3!3- + Cl- + 3H2O
A) Determine the order of each reactant.
B) determine the value of the rate constant for the formation of I3-.
C) What would be the initial rate of formation of I3 (in units of M/s) when the following initial concentrations were used?
[I-]= 2.00x10-3M, [ClO3-]= 2.00x10-3M, [H+]= 3.00x10-3M
D)Under the conditions specified in part C, what would be the initial rate of formation of chloride ion for this rection?
run no 0.0100M KI (mL) 00100M KClO3 (mL) 0.0100M HCl (mL) H2O (mL) Total Volume (mL) Initial Rate= [I3-]/t (M/s) 1 5.00 5.00 5.00 85.00 100.00 0.00170 2 5.00 10.00 5.00 80.00 100.00 0.00340 3 15.00 10.00 5.00 70.00 100.00 0.0306 4 15.00 10.00 10.00 65.00 100.00 0.0612 Consider this reaction and the experimental quantities given in the table. A) Determine the order of each reactant. B) determine the value of the rate constant for the formation of I3-. C) What would be the initial rate of formation of I3 (in units of M/s) when the following initial concentrations were used? [I-]= 2.00x10^-3M, [ClO3-]= 2.00x10^-3M, [H+]= 3.00x10^-3M D)Under the conditions specified in part C, what would be the initial rate of formation of chloride ion for this rection?Explanation / Answer
From the table it is clear that
order of the reaction with respect to I- =2
order of the reaction w.r.t ClO3- =1
and order of the reation w.r.t H+=1
rate of formation of I3 (r)= 1/3 dI3 / dt=k [I-] 2[ClO3-]1[H+]1
dI3 / dt =3k[I-] 2[ClO3-]1[H+]1
0.0017=3 k [0.01]2[0.01]1[0.01]1
rate constant k= 1.7*105 mol-3 L3 sec-1
iii) rate of formation of I3 (r)= dI3 / dt=3k [I-] 2[ClO3-]1[H+]1
dI3 / dt= 3* 1.7* 10^5 [2*10^-3]2 [2*10^-3][3*10^-3]
= 122.4*10^--7
=1.224*10^-6 M/s
iv) formation of chloride = dCl/dt=k [I-] 2[ClO3-]1[H+]1
= 1.7*10^5 * 24*10^-12= 1.7* 10^-7 M/s