The decomposition of hydrogen peroxide in an aqueous solution is a first order reaction. It can be studied by titrating quickly 10 mL portions of reactions mixture at various times from the t = 0 of reaction against a standard solution of KMnO 4 . Volume of KMnO 4 solution used in each case is proportional to the remaining concentration of H 2 O 2 .
From the following data calculate the rate constant of the reaction,
Time (seconds) 0 600 1200
KMnO 4 solution used (mL) 22.8 13.8 8.2
Text Solution
Verified by ExpertsCHECK THE SOLUTION.
Here a = 22.8, a – x = Vol. of KMnO 4 used at various times t.
At time 600 seconds : K = 
log 
= 0.000837
At time 1200 seconds : K = 
log 
= 0.000852
Average value of K = 
= 0.000844 ×10 –4 sec –1
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