The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way:

OCl−+I−→OI−+Cl−.

This rapid reaction gives the following rate data:

[OCl−](M) [I]−(M) Rate (M/s)
1.5×10^−3 1.5×10^−3 1.36×10^−4
3.0×10^−3 1.5×10^−3 2.72×10^−4
1.5×10^−3 3.0×10^−3 2.72×10^−4

a. Write the rate law for this reaction.
b. Calculate the rate constant with proper units.
c. Calculate the rate when [OCl-]= 1.8×10^3 M and [I-]= 6.0×10^4 M .

a) The rate law for this reaction:

b)The rate constant of the reaction is .

c)The rate of the reaction at given concentration will be .

Explanation:

a) Rate law of the reaction is given by :

1) Rate of the reaction when and .

..[1]

2) Rate of the reaction when and .

..[2]

3) Rate of the reaction when and .

..[3]

[1] ÷ [2]

On solving the equation we get value of x :

x = 1

[1] ÷ [3]

On solving the equation we get value of y :

y = 1

The rate law for this reaction:

b)

Rate of the reaction when and .

The rate constant of the reaction is .

c)

Let the rate of the reaction when and be R.

The rate of the reaction at given concentration will be .

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong