Odine atoms will combine to form I2 in liquid hexane solvent with a rate constant of 1.5×1010L/mol⋅s. The reaction is second order in I . Since the reaction occurs so quickly, the only way to study the reaction is to create iodine atoms almost instantaneously, usually by photochemical decomposition of I2. Suppose a flash of light creates an initial [I] concentration of 2.00×10−2 M . How long will it take for 94% of the newly created iodine atoms to recombine to form I2? Express your answer using two significant figures.

The time taken is  

Explanation:

From the question we are told that

    The  rate constant is  

    The initial concentration of iodine atom  is  

Generally the integrated  rate law for a second order reaction is  mathematically represented as

Where is the concentration of the remaining iodine atom  after the recombination which is mathematically evaluated as

      [100%  - 94%]

The reason for the 94%  is that we are told from the question that only 94% of the iodine atom recombined

=>  [6%]

=>  

substituting values

So

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.