Question

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.

Answer 1

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

Answer 2

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 $cm^3$

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]$_2$ (cyanogen is a toxic gas)