Which volume of oxygen, at room temperature and pressure, is needed for complete combustion

of 1.0mol of methylpropan-1-ol?

A 108dm3 B 144dm3 C 156dm3 D 288dm

The molecular formula of methylpropan-1-ol is C4H10O, so the complete combustion equation is: C4H10O + 6O2 - - > 4CO2 + 5H2O. This mean to completely combust 1.0mol of methylpropan-1-ol, 6 mol of O2 is required. Molar mass of O2 is 32 g/mol, so 32g/mol x 6mol = 192 g of O2 is required. At room temperature and pressure, the density of O2 is 1.3315 g/L (this can be obtained by density of gas = P/RT). So the volume of O2 = mass/density = 192g/1.3315 (g/L) = 144 L = 144 dm3. The answer is B.

To determine the volume of oxygen needed for the reaction, we need to know the chemical formula of the fuel in order to know the chemical reaction. Methylpropan-1-ol has a formula of C4H10O. The chemical reaction would be:

C4H10O + 6O2 = 4CO2 + 5H2O

We calculate volume as follows:

1 mol C4H10O (6 mol O2 / 1 mol C4H10O) (22.4 L O2 / 1 mol O2) = 134.4 L O2 needed or 134.4 dm^3

Therefore, the closest value would be B, 144 dm^3.