suppose we were able to meausre the amout of oxygen gas form

suppose we were able to meausre the amout of oxygen gas formed in units of moles/L, and the rate of formation of oxygen was found to be 0.125M/s.

reaction: H2O2(l) ---> H2O (l) + O2 (g)

a.) using the rate law for this reaction and the units associated with each variable, show what the derived units for the rate law constant k would be.

b.) What would be the rate of decomposition of the hydrogen peroxide? Explain your answer.

Solution

a)

it is clearly known that it is first order reaction . so for first order only time-1 units are left finally for rate constant

rate constant = 1/sec    or     sec^-1

b)

H2O2(l) ---> H2O (l) + 1/2 O2 (g)

from above equation ;   rate   = - d[H2O2] / dt = 1/2 *d[O2] / dt

rate of decomposition of the hydrogen peroxide = - d[H2O2] / dt = 1/2 *d[O2] / dt

                                                                             = 1/ 2* 0.125

                                                                             = 0.0625 M / s