When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 13.2 g of carbon were burned in the presence of 48.8 g of oxygen, 13.6 g of oxygen remained unreacted. What mass of carbon dioxide was produced?
Express your answer to one decimal place and include the appropriate units.
C(s) + O2(g) ==> CO2(g)
mols C = grams/atomic mass = 13.2/12 = 1.1 initially.
48.8 g O2 initially - 13.6 g O2 remaining = 35.2 g O2 used.
mols O2 used = g/molar mass = 35.2/32 = 1.1
The equation tells you that 1.1 mols C will use 1.1 mols O2 to produce 1.1 mols CO2.
g CO2 = mols CO2 x molar mass CO2 = 1.1 x 44 = ? grams CO2.
To find the mass of carbon dioxide produced, we need to calculate the mass of oxygen consumed in the reaction and then use the stoichiometry of the reaction to determine the mass of carbon dioxide produced.
1. Calculate the mass of oxygen consumed:
Mass of oxygen consumed = Initial mass of oxygen - Final mass of oxygen
Mass of oxygen consumed = 48.8 g - 13.6 g
Mass of oxygen consumed = 35.2 g
2. Use the stoichiometry of the reaction to find the mass of carbon dioxide produced:
From the balanced chemical equation, we know that the reaction consumes 1 mole of carbon and 1 mole of oxygen to produce 1 mole of carbon dioxide. The molar mass of carbon dioxide is 44.01 g/mol.
The molar ratio between carbon and carbon dioxide is 1:1, so the mass of carbon dioxide produced is equal to the mass of carbon consumed.
Mass of carbon dioxide produced = Mass of carbon consumed = 13.2 g
Therefore, the mass of carbon dioxide produced is 13.2 g.
Answer: 13.2 g of carbon dioxide.