When the Carbon reacts with oxygen it produce CO₂. This can be depicted by the below equation.
C + O₂ → CO₂. By the given process, 57.2 g of CO₂ are produced.
It has been mentioned that when 15.6 g of C reacts with 52.1 g of O₂ , then 10.5 g of O₂ remains unreacted. It indicates that Carbon is the limiting reagent and hence the amount of CO₂ produced is based on the amount of Carbon burnt.
C + O₂ → CO₂
In the given equation , 1 mole of carbon reacts with the 1 mole of O₂ to produce 1 mole of CO₂.
In the case 15.6 g of Carbon reacts with 52.1 of O₂ to produce the "x" g of CO₂.
No of moles of a substance = mass of the substance/molar mass of substance
No of moles of carbon = 15.6 /12= 1.3 moles
No of moles of O₂ = Mass of reacted O₂/Molar mass of O₂.
No of moles of O₂ = (Total mass of O₂ burned - Mass of unreacted O)/32
No of moles of O₂ = (52.1-10.5) ÷ 32 = 1.3 moles.
Hence as already discussed 1 mole of Carbon reacts with 1 mole of O₂ to produce 1 mole of CO₂. In this case 1.2 moles of carbon reacts with 1.3 moles of O₂ to produce 1.3 moles of CO₂.
Moles of carbon dioxide = Mass of CO₂ produced /Molar mass of CO₂
Mass of CO₂ produced(x) = Moles of CO₂ ×Molar mass of CO₂
Mass of CO₂ produced(x) = 1.3 x 44 = 57.2 g
Thus 57.2 g of CO₂ is produced.
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