How many grams of carbon dioxide can form when a mixture of 3.20 g ethylene (C2H4) and 5.90 g of oxygen is ignited, assuming complete combustion to form carbon dioxide and water?
Give the answer again with the correct number of significant figures.
C2H4 (g) + 3O2(g) ------------------> 2CO2(g) + 2H2O(g)
no of moles of C2H4 = W/G.M.Wt
= 3.2/28
= 0.1143 moles
no of moles of O2 = W/G.M.Wt
= 5.9/32
= 0.184 moles
C2H4 (g) + 3O2(g) ------------------> 2CO2(g) + 2H2O(g)
1 moles of C2H4 react with 3 moles of O2
0.1143 moles of C2H4 react with = 3*0.1143/1 = 0.3429 moles of O2 is required
O2 is limiting reactant
3 moles of O2 react with excess of C2H4 to gives 2 moles of CO2
0.184 moles of O2 react with excess of C2H4 to gives = 2*0.184/3 = 0.1226 moles of CO2
mass of CO2 = no of moles * gram molar mass
= 0.1226*44 = 5.4g of CO2 >>>>>answer
How many grams of carbon dioxide can form when a mixture of 3.20 g ethylene (C2H4)...
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