Please calculate the number of mols of oxygen gas produced per second

Remember PV=nRT and that you must account for the partial pressure of water vapour.

The reactions conditions are:

Atmospheric pressue:102.6 kPa;

Temperature:290 K

Partial pressure of water vapour:1.94 kPa.

The reaction is:

Volume of 6% H2O2 (mL):10.0

Volume of distilled water (mL):0.0

Volume of 1.0 M NaI (mL):10.0

Volume of distilled water (mL):0.0

O2 production in 60 s (mL):151.0

What I have done thus far is rearranged the Ideal Gas Law in order to get the number of mols

n = PV/RT

Is this the correct first step

Also, I have substituted the following values into the equation:

P = 102.6 kPa

V = ?

R = 8.3145 J/mol K

T = 290 K

Thank you for any help it is greatly appreciated.