Question

Q14) 0.1931 g of diamond gave 0.704 g of carbon dioxide on complete combustion. Calculate the percentage purity of diamond.
plss solve its tooo difficult i will mark brainliest if ans is correct

Answer 1

Given:

The mass of diamond = 0.1931 gm

The mass of carbon dioxide formed = 0.704 gm

To Find:

The percentage purity of the diamond.

Calculation:

- The combustion of diamond is given as:

C + O2 → CO2

⇒ The mass of diamond required to evolve 44 gm of CO2 = 12 gm

⇒ The mass of diamond required to evolve 0.704 gm of CO2 = (12/44) × 0.704

⇒ The mass of diamond in the impure sample = 0.192 gm

- Percentage purity = (Mass of the pure compound in the sample/Total mass of impure sample) × 100

⇒ Percentage purity = (0.192/0.1931) × 100

⇒ Percentage purity = 99.43 %

- So, the percentage purity of the diamond is 99.43 %.