A toxic gas, A, consists of 53.8% nitrogen and 46.2% carbon by mass. At
273 K and 1.01 x 105 Pa, 1.048 g of A occupies 462 cm3. Determine the empirical
formula of A. Calculate the molar mass of the compound and determine its
molecular structure.
Answers
Answer:
The empirical formula of A is CN
Explanation:
You divide the percentages of the various elements by their relative atomic masses then you divide throughout by the smallest number
Given,
A toxic gas -> A
The composition of A = 53.8% nitrogen
46.2% carbon
at 273 K and 1.01 × 105 Pa.
the volume of 1.048 g of A = 462
To find,
The empirical formula of A
The molar mass and the molecular structure of A.
Solution,
dividing the given percentage of constituent elements by their molar masses,
for N -> 53.8/14 = 3.84
for C -> 46.2/12 = 3.85
∴ they are in the ratio of 1:1
⇒ Empirical formula = CN
(there are no H atoms present, which eradicates the possibility of the compound being HCN)
So, we can say,
∵ Since it's the empirical formula must be CN
∴ The molecular formula must be [CN] (cyanogen is a toxic gas)