(a) Calculate the number of moles and the number of molecules present in 1.4 g of ethylene gas. What is the volume occupied by the same amount of ethylene?
(b) What is the vapour density of ethylene?

Question

(a) Calculate the number of moles and the number of molecules present in 1.4 g of ethylene gas. What is the volume occupied by the same amount of ethylene? (b) What is the vapour density of ethylene?

KnowledgeBoat · Accepted Answer

Gram molecular mass of C₂H₄ = 2(12) + 4(1) = 24 + 4 = 28 g As, 28 g of C₂H₄ = 1 mole 1.4 g of C₂H₄ = x 1.4 = 0.05 moles 1 mole = 6 × 10²³ molecules 0.05 moles = 6 × 10²³ x 0.05 = 3 x 10²² molecules Hence, no. of moles is 0.05 and no. of molecules is 3 x 10²². Vol. occupied by 1 mole = 22.4 lit Vol. occupied by 0.05 moles = 22.4 x 0.05 = 1.12 lit. Hence, vol. occupied is 1.12 lit (b) Hence, vapour density is 14

Chemistry

(a) Calculate the number of moles and the number of molecules present in 1.4 g of ethylene gas. What is the volume occupied by the same amount of ethylene?
(b) What is the vapour density of ethylene?

Mole Concept

Related Questions

Given that the relative molecular mass of copper oxide is 80, what volume of ammonia (measured at STP) is required to completely reduce 120 g of copper oxide? The equation for the reaction is:
3CuO + 2NH₃ ⟶ 3Cu + 3H₂O + N₂

Chemistry

(a) Calculate the number of moles and the number of molecules present in 1.4 g of ethylene gas. What is the volume occupied by the same amount of ethylene?(b) What is the vapour density of ethylene?

Mole Concept

Related Questions

Given that the relative molecular mass of copper oxide is 80, what volume of ammonia (measured at STP) is required to completely reduce 120 g of copper oxide? The equation for the reaction is:3CuO + 2NH3 ⟶ 3Cu + 3H2O + N2

(a) Calculate the number of moles and the number of molecules present in 1.4 g of ethylene gas. What is the volume occupied by the same amount of ethylene?
(b) What is the vapour density of ethylene?

Given that the relative molecular mass of copper oxide is 80, what volume of ammonia (measured at STP) is required to completely reduce 120 g of copper oxide? The equation for the reaction is:
3CuO + 2NH₃ ⟶ 3Cu + 3H₂O + N₂