A certain compound contains C, H and O. One molecule of the compound is known to contain 2 atoms of O, and the number of atoms of H is two times the number of atoms of C per molecule. when a quantity of the compound is burned completely in O2 to form CO2 and H2O as the only products, .375 mol of O2 is consumed and .3 mol of H2O is formed. Calculate the chemical formula of the compound

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

1 is the answer to this problem

catya that's not even a b or c

the answer your looking for is c).