# What mass of oxgyen is comsumed by the complete combustion of 21.0grams of ethylene?

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C2H4(ethylene)+3O 2 →2CO 2 +2H 2O

ethylene)+3O 2 →2CO 2 +2H 2OTo oxidise 1 mol of ethylene we require 3 moles of Oxygen

ethylene)+3O 2 →2CO 2 +2H 2OTo oxidise 1 mol of ethylene we require 3 moles of Oxygen∴ For oxidising 28g of ethylene we require (3×32)g of oxygen

ethylene)+3O 2 →2CO 2 +2H 2OTo oxidise 1 mol of ethylene we require 3 moles of Oxygen∴ For oxidising 28g of ethylene we require (3×32)g of oxygen∴ For oxidising 2800g (2.8kg) of ethylene we require (96×100)g of oxygen

ethylene)+3O 2 →2CO 2 +2H 2OTo oxidise 1 mol of ethylene we require 3 moles of Oxygen∴ For oxidising 28g of ethylene we require (3×32)g of oxygen∴ For oxidising 2800g (2.8kg) of ethylene we require (96×100)g of oxygen∴For oxidising 2.8kg of ethylene we require 9600g of oxygen

ethylene)+3O 2 →2CO 2 +2H 2OTo oxidise 1 mol of ethylene we require 3 moles of Oxygen∴ For oxidising 28g of ethylene we require (3×32)g of oxygen∴ For oxidising 2800g (2.8kg) of ethylene we require (96×100)g of oxygen∴For oxidising 2.8kg of ethylene we require 9600g of oxygenSo to oxidise 2.8kg of ethylene we require 9.6kg of oxygen.

ethylene)+3O 2 →2CO 2 +2H 2OTo oxidise 1 mol of ethylene we require 3 moles of Oxygen∴ For oxidising 28g of ethylene we require (3×32)g of oxygen∴ For oxidising 2800g (2.8kg) of ethylene we require (96×100)g of oxygen∴For oxidising 2.8kg of ethylene we require 9600g of oxygenSo to oxidise 2.8kg of ethylene we require 9.6kg of oxygen.Hence option C is correct.

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