Question

Consider the decomposition of hydrogen peroxide reaction. If the rate of decomposition of hydrogen peroxide at a particular temperature is determined to be 0.098 mol/(L·s), what are the rates of reaction with respect to the products of the decomposition reaction?

Answer 1

0.049 mol/L.s

Step-by-step explanation:

The decomposition of hydrogen peroxide is:

`H_2O_2 \to H_2O + (1)/(2)O_2`

`Rate = -(\Delta [H_2O_2])/(\Delta t)= (\Delta [H_2O_2])/(\Delta t)= ( 2 \Delta [H_2O_2])/(\Delta t)`

The rate of decomposition reaction = the rate of formation of
`H_2O` = 0.098 mol/L.s

∴

Rate of formation of
`O_2`
`= ( rate \ of \ reaction )/(2)`

`= ( 0.098 )/(2)`

= 0.049 mol/L.s