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Recall the demonstration from lecture where we "burned" ethanol in a 2-gallon drum to produce carbon...

Recall the demonstration from lecture where we "burned" ethanol in a 2-gallon drum to produce carbon dioxide and water. The unbalanced equation is: C2H5OH(g) + O2(g) → CO2(g) + H2O(l)

If 2.00g of ethanol reacts with 10.0g of oxygen, how many moles of carbon dioxide and how many moles of water are produced?

What is the total volume of gas present (in L) after the reaction is complete assuming the reaction takes place at 1.00 atm and 25°C?

Prove that mass has been conserved in this reaction (within three significant figures). What mass of ethanol is present before the reaction takes place?

What mass of oxygen is present before the reaction takes place?

What is the total mass of substances present before the reaction takes place?

What mass of carbon dioxide is present after the reaction takes place?

What mass of water is present after the reaction takes place?

What mass of leftover reactant is present after the reaction takes place?

What is the total mass of substances present after the reaction takes place?

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C ₂ H 5 OH cg, +30 2(g) 200, Cg , + 3H2O ces 0.043 0.312 C2H5OH is to 0.043 LR 0.312 (0.312-0. 129) 2x0.043 3x0.043 t o 0 .18Mass after reaction, = (0.183) X32 + (0.086) x 44 + 0.129 (18) - 5.856 +3.784 + 2.322 = 11.962 9. 4 nog of O2 is present befoPlease like the solution.Feel free to ask any doubt in comments.

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