please answer my question as soon as possible. i have my exams tomorrow
a)Combustion of 0.2000g of vitamin C gives 0.2998g of CO2
and 0.819g of H2O. What is the empirical formula of vitamin C?
b)4 litres of water are added to 2L of 6 molar HCl solutions.
What is the molarity of resulting solution?
a)
Mass of water produced in this reaction must be 0.0819g and not 0.819g.
Given that vitamin C on combustion gives carbon dioxide and water.Let vitamin C is X.
X (s) + O2(g) CO2 (g) + H2O (l)
0.2000 g 0.2998g 0.0819g
Molar mass of CO2 = 12 + 216= 44 g
Amount of carbon in 44 g CO2 = 12 g
Amount of carbon in 0.2998g CO2 = g =0.0818 g
Molar mass of H2O = 12 + 16= 18 g
Amount of hydrogen in 18 g H2O = 2 g
Amount of hydrogen in 0.0819 g H2O = g =0.0091 g
Percentage of carbon in fuel gas = = 40.9 %
Percentage of hydrogen in compound = = 4.55 %
Thus Percentage of oxygen in the compound= 100 - (40.9 + 4.55) = 54.55 %
Thus the simple ratio of C:H:O is 3:4:3
Thus empirical formula of the compound = C3H4O3
b)
Thus now the molarity of the solution is 2 M
Mass of water produced in this reaction must be 0.0819g and not 0.819g.
Given that vitamin C on combustion gives carbon dioxide and water.Let vitamin C is X.
X (s) + O2(g) CO2 (g) + H2O (l)
0.2000 g 0.2998g 0.0819g
Molar mass of CO2 = 12 + 216= 44 g
Amount of carbon in 44 g CO2 = 12 g
Amount of carbon in 0.2998g CO2 = g =0.0818 g
Molar mass of H2O = 12 + 16= 18 g
Amount of hydrogen in 18 g H2O = 2 g
Amount of hydrogen in 0.0819 g H2O = g =0.0091 g
Percentage of carbon in fuel gas = = 40.9 %
Percentage of hydrogen in compound = = 4.55 %
Thus Percentage of oxygen in the compound= 100 - (40.9 + 4.55) = 54.55 %
Element | Atomic mass of element | Percentage | Moles of the constituents | Molar ratio | Simple whole number ratio |
C | 12 | 40.9 | |||
H | 1 | 4.55 | |||
O | 16 | 54.55 |
Thus the simple ratio of C:H:O is 3:4:3
Thus empirical formula of the compound = C3H4O3
b)
Thus now the molarity of the solution is 2 M