Hi everyone,
I need help on calculating the volume of oxygen that is required to oxidise a dihydroxystillbene molecule (mass= 35mg, MW=430.09g/mol) into a diquinone methide molecule
So far I have calculated that 35 mg of dihydroxystillbene is equal to 0.082 mmol
A dihydroxystillbene molecule has 2 hydroxy groups on it, so theoretically for 1 mol of a dihydroxystillbene to be oxidised 2 mol of oxygen is required
So for 0.082 mmol of dihydroxystillbene to be oxidised, 0.164 mmol of oxygen is required
then using the ideal gas equation PV=nRT
V= 0.000164mol x8.314 JK-1mol-1 x 298K/ 101.325Pa
V = 0.00401 m^3
Is this correct???