I'm not sure this is kinetics, more stoichiometry. How much hydrogen peroxide do you have? How much oxygen can that produce from the balanced equation?
Well there is 30ml of H202 solution at 0.2 mol L-1.
Using n = c/v
n = 0.2 mol L-1 / 0.030 L
n = 6.67 moles of H2O2
The number of moles of O2 should be half of H2O2.
As 2H202 ---> 2H20 + O2 therefore O2 = 6.67 mol / 2
O2 = 3.33 moles of Oxygen produced.
To find the volume for Oxygen we can use the equation: n1v1 = n2v2
(6.67 mol * 0.030 L) / (3.33 * V2)
V2 = 0.2001 / 3.33
V2 = 0.060 L
V2 = 60 ml
Therefore the oxygen produced is 60 ml.
Is this correct? I just realised i typed out the wrong question.