Question

9. How many grams of CO2 will be produced if 32.10 g of C2H4 is combusted in the presence of 64.00 g of O2 and the reaction yield is 93.70 % C H4 (g) O2(g) CO2 (g) H2O () a) 58.68 g b) 54.98 g c) 123.7 g d) 18.02 g

Answer 1

The balanced chemical reaction is given by
C2H4(g)     + 3O2(g)    -------->      2CO2(g)      + 2H2O(l)

   1.0 mole     3.0 mole                  2.0 mole      2.0 mole

The number of moles C2H4, n= 32.10/28 = 1.15 mole

The number of moles O2, n= 64/32 = 2.0 mole

Therefore, oxygen (O2) is the limiting reagent and the amount of CARBON DIOXIDE gas produced depends on the limiting reagent only

3.0 mole of oxygen produces 2 moles of CO2 gas

2.0 moles of oxygen produces 2*2/3 = 1.33 moles of CO2 gas

The mass of CO2 gas produced = 58.52 grams (theoretically)

But, given percent yield of the reaction = 93.70%

The actual mass of CO2 gas produced 58.52*93.70/100 = 54.98 grams