Formic acid, HCHO2, burns in oxygen to form carbon dioxide and water as follows:
HCHO2 (aq) + O2 (g) → 2CO2 (g) + 2H2O (l).
If a 3.15 gram sample of formic acid was burned in 15.00 grams of oxygen, what mass of carbon dioxide would be produced?
Answers
Formic acid, HCHO2, burns in oxygen to form carbon dioxide and water as follows: HCHO2 (aq) + O2 (g) → 2 CO2 (g) + 2 H2O (l).
The reaction taking place is:
HCHO2 (aq) + O2 (g) → 2CO2 (g) + 2H2O
=> So, 1 part of HCOOH reacts with 1 part of O2 to give 2 parts of CO2 and 2 parts of water.
=> We can assume that 3.15 grams of HCOOH was burnt completely in the required amount of oxygen.
=> Molar mass of HCOOH = 1 + 12 + 2*16 + 1 => 2+12+32
=> 46 grams per mole.
=> So, 3.15 grams is 3.15/46 moles => 0.068 moles of HCOOH.
=> So, from the equation, 1 part of HCOOH = 0.068 moles.
=> So, 2 parts of CO2 is 2*0.068 moles => 0.136 moles of CO2.
=> Molar mass of CO2 = 12 + 2 x 16 => 12+32 => 44 grams per mole.
=> Hence, 0.136 moles of CO2 will have a mass of 44*0.136 =>5.984 g
Hence, the mass of Carbon dioxide produced will be 5.984 grams.