Hi can someone please help with this question, or atlest direct me in the right direction. Please and thank you.
The initial rate of reaction
H2O2(aq) --> H2O (l) + 1/2 O2(g)
is found to be1.7*10^-3 M/s . Assume that this rate holds for 2 minutes. Start with 165ml of 1.55M H2O2 (aq) at t=0 .
How many milliliters of O2(g) measured at 24 degress celsius and 759 , are released from solution in the first minute of the reaction?
Is the rate 1.7*10^-3 mol. H2O2/s or 1.7*10^-3 mol. O2/s ?? It makes a difference.
Multiply the rate by 60 s to get moles of H2O2 or O2 formed. If the rate is moles H2O2/s, you must divide the moles you get by 2 to get moles of O2.
Next, use the Ideal Gas Law, PV = nRT, to get V in liters.
Finally, convert the liters to mLs.