Question

on complete combustion 0.858g of compound (x) gives 2.63g of carbon dioxide and 1.27g of water . calculate the empirical formula of the compound​

Answer 1

Answer:

mass of CO2 = 2.630 g or since the molar mass of CO2 is 44g / mole we have

0.05976 moles of CO2 since there is 1 mole so C in CO2

we have 0.05976 moles of C or 0.718 g of C

mass of H2O = 1.280 g or since the molar mass of wateris 18 g / mol we have

0.07105 moles of H2O since there are2 moles of H in 1 moles of H2O =

0.14210 moles of H or 0.143 g of H

molar ratio of C : H = 0.05976 : 0.14210

mass of C+H = 0.861 g

or after dividing by the smallest 0.05976

molar ratio of C : H = 1.000 : 2.378

multiply by 3 to get whole numbers 3.000 7.134 :

empirical formula is C3H7

so minimum molar mass is 43g / mol