Question

2. Combustion of 8.652 g of a compound containing C, H, O and N in air yields 11.088 g

CO2, 3.780 g H₂O, and 3.864 g NO2. This is chapter 3!!!
How many grams of C, H, and N are contained in the sample? (6 points)
How many grams of O are contained in the sample? (2 points)
What is the simplest formula of the compound? (3 points)
If the molar mass of the compound lies between 200 and 300, what is its molecular
formula? (3pts)
Write and balance a chemical equation for the combustion of the compound. (2pts)

Answer 1

Step-by-step explanation:

Answer:- C = 3.024 g, H = 0.42 g, N = 1.176 g and O = 4.032 g

Solution:- The compound contains C, H, N and O. On combustion, all the carbon is converted to carbon dioxide, All hydrogen is converted to water and all the nitrogen is converted to nitrogen dioxide.

From the grams of all these, we could calculate their moles and then using mol ratio of these products and the number of moles of C, H and N present in them, we calculate the moles of C, H and N respectively. Further, these moles are converted to grams. On subtracting the sum of grams of C, H and N from the mass of the sample, the mass of oxygen is calculated.

The calculations are as follows:

Calculations for the grams of C:-

= 3.024 g C

Calculations for the grams of H:-

= 0.42 g H

Calculations for the grams of N:-

= 1.176 g N

Mass of the compound is given as 8.652 g. Now we could calculate the grams of oxygen as:

mass of oxygen = 8.652 - (3.024 + 0.42 + 1.176)

= 8.652 - 4.62

= 4.032 g

So, 8.652 grams of the compound contains 3.024 g of C, 0.42 g of H, 1.176 g of N and 4.032 g of O.