The combustion reaction of acetylene gas is represented by this equation:
2C2H2(g) + 5 O2(g) ==> 4CO2(g) + 2H2O(g)
How many grams of CO2 and grams of H2O are produced when 52.0g C2H2 burns in oxygen?
To find the amount of CO2 and H2O produced, we need to use the balanced equation provided.
From the balanced equation:
2 moles of C2H2 produce 4 moles of CO2
2 moles of C2H2 produce 2 moles of H2O
First, let's calculate the moles of C2H2 using its molar mass:
Molar mass of C2H2:
C: 2 atoms x 12.01 g/mol = 24.02 g/mol
H: 2 atoms x 1.008 g/mol = 2.016 g/mol
Total molar mass = 24.02 g/mol + 2.016 g/mol = 26.036 g/mol
Now, we can calculate the moles of C2H2 using its given mass:
Moles of C2H2 = 52.0 g / 26.036 g/mol ≈ 1.995 mol
Since the ratio of CO2 to C2H2 is 4:2, and the ratio of H2O to C2H2 is 2:2, we can calculate the moles of CO2 and H2O produced:
Moles of CO2 = 1.995 mol x (4 mol CO2 / 2 mol C2H2) = 3.99 mol
Moles of H2O = 1.995 mol x (2 mol H2O / 2 mol C2H2) = 1.995 mol
Finally, we can convert the moles of CO2 and H2O to grams using their respective molar masses:
Molar mass of CO2:
C: 1 atom x 12.01 g/mol = 12.01 g/mol
O: 2 atoms x 16.00 g/mol = 32.00 g/mol
Total molar mass = 12.01 g/mol + 32.00 g/mol = 44.01 g/mol
Molar mass of H2O:
H: 2 atoms x 1.008 g/mol = 2.016 g/mol
O: 1 atom x 16.00 g/mol = 16.00 g/mol
Total molar mass = 2.016 g/mol + 16.00 g/mol = 18.02 g/mol
Now, let's calculate the mass of CO2 and H2O:
Mass of CO2 = 3.99 mol x 44.01 g/mol ≈ 175.6189 g ≈ 175.62 g (rounded to 2 decimal places)
Mass of H2O = 1.995 mol x 18.02 g/mol ≈ 35.9919 g ≈ 36.00 g (rounded to 2 decimal places)
Therefore, when 52.0 g of C2H2 burns in oxygen, approximately 175.62 grams of CO2 and 36.00 grams of H2O are produced.
To determine the amount of CO2 and H2O produced when 52.0g of C2H2 burns, you need to calculate the moles of C2H2, and then use the stoichiometry of the balanced equation to find the moles of CO2 and H2O produced. Finally, convert the moles of CO2 and H2O to grams using their respective molar masses.
1. Calculate the moles of C2H2:
To calculate the moles, divide the given mass of C2H2 (52.0g) by its molar mass. The molar mass of C2H2 is calculated by adding the atomic masses of its constituent elements (carbon and hydrogen):
C2H2 molar mass = (2*atomic mass of carbon) + (2*atomic mass of hydrogen)
= (2*12.01) + (2*1.01)
= 26.04 g/mol
Moles of C2H2 = 52.0g / 26.04 g/mol
2. Use the stoichiometry of the balanced equation to determine the moles of CO2 and H2O produced:
According to the balanced equation, the mole ratio between C2H2 and CO2 is 2:4, and the mole ratio between C2H2 and H2O is 2:2.
Moles of CO2 = Moles of C2H2 * (4 moles CO2 / 2 moles C2H2)
Moles of H2O = Moles of C2H2 * (2 moles H2O / 2 moles C2H2)
3. Convert the moles of CO2 and H2O to grams using their respective molar masses:
The molar mass of CO2 is calculated by adding the atomic masses of carbon and oxygen:
CO2 molar mass = (1*atomic mass of carbon) + (2*atomic mass of oxygen)
= 12.01 + (2*16.00)
= 44.01 g/mol
The molar mass of H2O is calculated by adding the atomic masses of hydrogen and oxygen:
H2O molar mass = (2*atomic mass of hydrogen) + (1*atomic mass of oxygen)
= (2*1.01) + 16.00
= 18.02 g/mol
Grams of CO2 = Moles of CO2 * CO2 molar mass
Grams of H2O = Moles of H2O * H2O molar mass
By performing these calculations, you can determine the grams of CO2 and H2O produced when 52.0g of C2H2 burns in oxygen.