Question

Find mass of O2 required when 5.8g
of butane is burnt ?.
cuH10 + >CO2+H2o​

Answer 1

Answer:

0.65 mol.

Explanation:

= 0.10 mol.

The balanced equation for the combustion of butane is:

C4H10(g) + O2(g) → 4CO2(g) + 5H2O(l)

Hence, 13/2 moles of O2 are required and 4 moles of CO2 and 5 moles of H2O are.

produced for every mole of C4H10 which combusts. As 0.10 mol of C4H10 is.

present:

number of moles of O2 needed =

× 0.10 mol = 0.65 mol.