Below is data that Barney collected for a kinetic study investigated the effect

ID: 485840 • Letter: B

Question

Below is data that Barney collected for a kinetic study investigated the effect that hydroxide had on the reaction rate for the chemical reaction:

I - (aq) + OH- (aq) ----------> IO- (aq) + Cl- ( aq)

[OCl -] initial [OH-] Inital [ I-] Inital Inital rate (mol/L sec)

0.013 0.012 0.10 9.4 E^ -3

0.0026 0.012 0.10 1.87 E^ -2

0.0013 0.006 0.10 4.7 E^ -3

0.0013 0.018 0.10 1.4 E^ -2

0.0013 0.012 0.05 1.87 E ^ -2

0.0013 0.012 0.20 4.7 E ^ -3

0.0013 0.018 0.20 7.0 E ^ -3

From the above information in the table :

A. Determine the rate law for the chemical reaction

B. What is the overall rate order for the chemical reaction?

C. Determine the units for the rate constant (k)

D. Determine the numberical value for the the rate constant.

see 1st 2 rows
[OH-] constant
[I-] constant
[OCl-] doubles
rate also doubles
so, order of OCl- is 1

see 1st and 3rd row
[OCl-] constant
[I-] constant
[OH-] is halfed
rate also halfes
so, order of OH- is 1

see 5th and 6th row:
[OCl-] constant
[OH-] constant
[I-] becomes 4 times
rate becimes 1/4 times
so, order of I- is -1

A)
RATE law is:
rate = k [OCl-] [OH-] [I-]^-1

B)
overall order = 1 + 1 -1 = 1
Answer: 1

C)
for 1st order unit is s-1

Answer: s-1

D)
rate = k [OCl-] [OH-] [I-]^-1
put values from row 1
9.4*10^-3 = k * 0.013 * 0.012 * (0.10)^-1
k = 6.03

Answer: numerical value is 6.03

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