Ideal Gas Law question

Oxygen gas, generated by the reaction 2KClO3(s)==>2KCl(s)+3O2(g), is collected over water at 27C (300.15K) in a 2.00L vessel at a total pressure of 760 torr (1atm?). (the vapor pressure of water at (27C is 26.0torr). How many moles of oxygen are produced during the reaction?

The answer is 0.0784 Moles. But I have no clue how to get it.

I know
t= 300.15
r= 0.08205
v= 2.00L
for pressure, do i use 1atm?

please help. thanks

P = 760 torr - 26.0 torr = 734 torr x 101.325 kPa/760 torr = 97.8586184 kPa - partial pressure question
V = 2.00 L
n = ?
R = 8.314 kPa * L / mol * K (not 0.08205)
T = 300.15 K

n = PV / RT
n = (97.8586184)(2.00) / (8.314)(300.15)
n = 0.07842973 mol
n = 0.0784 mol = 7.84 x 10^-2 mol