Question

Complete combustion of 0.858 g of compound X gives 2.63 g of CO, and 1.28 g of H.O. The lowest
molecular mass X can have
(1) 43 g
(2) 86 g (3) 1299 (4) 1728
TL​

Answer 1

Answer:

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

2) 0.05976 moles of CO2 since there is 1 mole so C in CO2

3) 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 water is 18 g / mol

4) 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

5) molar ratio of C : H = 0.05976 : 0.14210

6) mass of C+H = 0.861 g

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

Answer 2

Answer:

c3h7

Explanation:

here we multiply by 3 to convert it in simple ratio