One chem question please

It reads: If 4.00 moles of gasoline are burned, what volume if oxygen is needed if the pressure is 0.953 atm, and the temperature is 35°C?

2 C8H18(l) + 25 O2(g)-----> 16 CO2(g) + 18 H2O (g)

*I know PV=nRT, but how do I incorporate the stoichiometry?

4 moles of C8H18 require 50 moles of O2.

This is the n in PV = nRT
V = nRT/P where
P = 0.953 atm
T = 308 degrees K
and R is the gas constant in L-atm/degree-mol

Plug and crank