A hydrocarbon containing C and H has 92.3 % C . When 39 g of hydrocarbon was completely burnt in O ₂, x moles of water and y moles of CO ₂ were formed. x moles of water is sufficient to liberate 0.75 moles of H ₂ with Na metal. What is the weight (in g ) of oxygen consumed? ( C =12 u ; H =1 u )

Step-by-step solution

empirical Ratio 1: 1 CH possible hydrocarbon C ₂ H ₂ C ₂ H ₂+ 5 2 O ₂ 2 CO ₂+ H ₂ O 2 H ₂ O +2 Na 2 NaOH + H ₂ 2 mole of H ₂ O gives one mol H ₂0.75 H ₂ Produced thus 1.5 ~mol H ₂ O used mass of 1.5 ~mol H ₂ O =1.5 18=17 On balancing and multiplying with 1.5 gathered 1.5 C ₂ H ₂+3.75 O ₂ 3 CO ₂+1.5 H ₂ O mass of O ₂ required =3.75 32=120 ~g gathered