a. A compound contains 52.2% C, 13.1 % H and Oxygen only. The vapour density of the compound is 23. Determine i. its empirical formula; ii. its molecular fo...

ai. %0   =  100 -  (52.2+13.1)
     =34.7
      C                H                             O
  52.2/12,       13.1/1,                   34.7/16
   4.35,         13.1,                         2.168
4.35/2.168,    13.1/2.168,         2.168/2.168
    2.00,              6.04,                    1
empirical formula  =  \(C_2H_6O\)

ii. 2 x vapour density = molecular mass
   2x23=46
(\(C_2H_6O)_n\) = 46
  [(12 x 2) + (1 x 6) + 16]n = 46
  46n = 46
      n = 1
  molecular formula = \(C_2H_6O\)

iii1. Hydroxyl

iii2. 

b. 2(\(C_6H_{10}O_5)_n + nH_2O --diatase→ nC_{12}H_{22}O_{11}\)
     \(C_{12}H_{22}O_{11} + H_2O --maltase→ C_6H_{12}O_6 + C_6H_{12}O_6\)
      \(C_6H_{12}O_6 --zymase→ 2C_2H_5OH + 2CO_2\)

ci. The reaction starts but the metal produces a layer of an oxide/aluminum oxide layer on its surface which is impermeable(to water) and stops the reaction.

ii. Add dilute hydrochloric acid to excess aluminum filter off the excess metal leave the filtrate in a warm place/evaporate the filtrate to the point of crystallization/leave it in the sun.

d. The flask is connected to the condenser and the solution is heated. The water vaporizes and is converted to(liquid)water in the condenser.