Using the balanced equation for the combustion of ethylene (C2H4), answer the following question
C2H4 + 302 - 2CO2 + 2H20
Be sure each of your answer entries has the correct number of significant figures.
Part 1 of 2
How many grams of CO2 are formed from 2.9 mol of C2H4?
Part 2 of 2
How many grams of H2O are formed from 0.13 mol of C2H4?
Part 1:
1. Calculate the molar mass of CO2:
12.01 g/mol (C) + 2(16.00 g/mol) = 44.01 g/mol
2. Use the stoichiometry of the balanced equation to convert moles of C2H4 to moles of CO2:
2.9 mol C2H4 x (2 mol CO2 / 1 mol C2H4) = 5.8 mol CO2
3. Calculate the mass of CO2 formed:
5.8 mol CO2 x 44.01 g/mol = 255 g CO2
Therefore, 255 grams of CO2 are formed from 2.9 mol of C2H4.
Part 2:
1. Calculate the molar mass of H2O:
2(1.01 g/mol) + 16.00 g/mol = 18.02 g/mol
2. Use the stoichiometry of the balanced equation to convert moles of C2H4 to moles of H2O:
0.13 mol C2H4 x (2 mol H2O / 1 mol C2H4) = 0.26 mol H2O
3. Calculate the mass of H2O formed:
0.26 mol H2O x 18.02 g/mol = 4.68 g H2O
Therefore, 4.68 grams of H2O are formed from 0.13 mol of C2H4.