Calculate the number of moles of oxygen gas produced from the completely catalyzed decomposition of 7.00ml sample of a 3.5% solution of H2O2. The density of the 3.5% solution of H2O2 is 1.01 g/ml.
Catalyst: simplest manganese(IV) oxide [used in nearly all schools and college experiments for this] even light will do .. this is why H2O2 is kept in dark bottles!
Answers & Comments
Verified answer
mass solution = 7.00 mL x 1.01 g/mL = 7.07 g
mass H2O2 =3.5 x 7.07 / 100 = 0.274 g
moles H2O2 = 0.274 g / 34.0148 g/mol = 0.00806
the ratio between H2O2 and O2 is 2 : 1
moles O2 = 0.00806 x 1 / 2 =0.00403
H2o2 Aq
For the best answers, search on this site https://shorturl.im/avF0M
Catalyst: simplest manganese(IV) oxide [used in nearly all schools and college experiments for this] even light will do .. this is why H2O2 is kept in dark bottles!