Answer:
the molecular formula of the compound is N2O4
Explanation:
- Find the empirical formula
mole of N present = mass of N divided by molar mass of N = 0.140/14 = 0.01 mole
mole of O present = mass of O divided by molar mass of O = 0.320/16 = 0.02 mole
Divide both by the smallest number of mole to determine the coefficient of each, the smallest number of mole is 0.01 thus:
quantity of N = 0.01/0.01 = 1
quantity of O = 0.02/0.01= 2
thus the empirical formula = NO2
- Now determine the molecular formula by finding the ratio of molecular formula and empirical formula
Molar mass of molecular formula = 92.02 amu = 92.02 g/mole
Molar mass of empirical formula NO2 = (14 + (16 x 2)) = 46 g/mole
the x factor = 92.02/46 = 2
Molecular formula = 2 x NO2 = N2O4
The balanced chemical reaction is expressed as:
M + F2 = MF2
To determine the moles of the element fluorine present in the product, we need to determine the moles of the product formed from the reaction and relate this value to the ratio of the elements in MF2. We do as follows:
moles MF2 produced = 0.600 mol M ( 1 mol MF2 / 1 mol M ) = 0.600 mol MF2
molar mass MF2 = 46.8 g MF2 / 0.6 mol MF2 = 78 g/mol
moles MF2 = 46.8 g ( 1 mol / 78 g ) = 0.6 mol
moles F = 0.6 mol MF2 ( 2 mol F / 1 mol MF2 ) = 1.2 moles F
speed = distance / time
v = d / t
If we simplify this and isolate t, then we get t = d / v
