The following figure represents the structural formula of a chemical compound.

Answer the questions given below:

(a) How many Carbon and Hydrogen atoms are present in the compound.

(b) Write the molecular and empirical formulae of the compound.

(c) Calculate the percentage composition of all the elements present in the compound. [At. wt. of C = 12, H = 1]

(a) 6 Carbon and 12 Hydrogen atoms are present.

(b) Its molecular formula is C₆H₁₂.
As the simplest ration between C and H is 1:2, hence the empirical formula is CH₂

(c) Relative molecular mass of C₆H₁₂
   = (6 x 12) + (1 x 12)
   = 72 + 12
   = 84 g

84 g of C₆H₁₂ contains 72 g of Carbon

∴ 100 g of C₆H₁₂ contains $\dfrac{72 \times 100}{84}$ g of Carbon

= $\dfrac{7200}{84}$ = 85.7 g of Carbon.

84 g of C₆H₁₂ contains 12 g of Hydrogen

∴ 100 g of C₆H₁₂ contains $\dfrac{12 \times 100}{84}$ g of Hydrogen

= $\dfrac{1200}{84}$ = 14.3 of Hydrogen.

∴ In C₆H₁₂, C = 85.7% and H = 14.3%