F.4 Chem,,,Reacting Masses***plz help!! ~_~

Question

1. A compound Y contains carbon, hydrogen and oxgen only. 0.62 g of Y was burnt in
excess oxygen. The masses of carbon dioxide and water produced were 0.88 g and
0.54 g respectively. Determine the empirical formula of Y.

Answer 1

mass of CO2 = 0.88 g
no. of mole of CO2 = 0.88 / (12+16X2) = 0.02
no. of mole of C = 0.02
mass of C in Y = 0.02 X 12 = 0.24 g
mass of H2O = 0.54
no. of mole of H2O = 0.54 / (1X2+16) = 0.03
no. of mole of H = 0.03 X 2 = 0.06
mass of H in Y = 0.06 X 1 = 0.06 g
mass of O in Y = 0.62 - 0.24 - 0.06 = 0.32


*************************** C ******************* H ****************** O
mass ****************** 0.24 **************** 0.06 **************** 0.32
no. of mole ********** 0.24/12 ************ 0.06 / 1 ************ 0.32 / 16
********************** = 0.02 ************** = 0.06 ************* = 0.02
simplest ratio ***** 0.02 / 0.02 *********** 0.06 / 0.02 ******** 0.02 / 0.02
********************** = 1 ********************* = 3 ************** = 1

empirical formula = CH3O

************ = nothing