how many grams of CO2 can be formed by the complete combustion of a 14.7 sample of C2H6 that is 92.4% pure?( assume the impurities contain no carbon)
balance the equation:
2C2H6+ 7O2 >> 4CO2 + 6H2O check that.
moles C2H6= (14.7g*.924)/molmassC2H6
massCO2= molesCO2*molmassCO2=2molesC2H6*molmassCO2
plug in the molar mass? is mass the same as molar mass?
To find out how many grams of CO2 can be formed by the complete combustion of C2H6, we need to calculate the number of moles of C2H6 and then use the stoichiometry ratios from the balanced chemical equation.
First, let's calculate the number of moles of C2H6:
Step 1: Calculate the molar mass of C2H6:
C: 12.01 g/mol x 2 = 24.02 g/mol
H: 1.01 g/mol x 6 = 6.06 g/mol
Total molar mass of C2H6 = 24.02 g/mol + 6.06 g/mol = 30.08 g/mol
Step 2: Calculate the moles of C2H6 using the given mass and the purity percentage:
Mass of C2H6 = 14.7 g x 0.924 = 13.5718 g
Moles of C2H6 = Mass of C2H6 / Molar mass of C2H6
= 13.5718 g / 30.08 g/mol
≈ 0.4513 mol
Now, let's use the stoichiometry ratios from the balanced chemical equation to calculate the moles of CO2 produced:
The balanced chemical equation for the combustion of C2H6 is:
C2H6 + 7/2 O2 -> 2 CO2 + 3 H2O
From the equation, we can see that 1 mole of C2H6 produces 2 moles of CO2. Therefore:
Moles of CO2 = 2 x Moles of C2H6
= 2 x 0.4513 mol
≈ 0.9026 mol
Finally, let's calculate the mass of CO2 formed:
Step 3: Calculate the mass of CO2 using the molar mass of CO2:
Molar mass of CO2 = 12.01 g/mol + (2 x 16.00 g/mol) = 44.01 g/mol
Mass of CO2 = Moles of CO2 x Molar mass of CO2
= 0.9026 mol x 44.01 g/mol
≈ 39.72 g
Therefore, approximately 39.72 grams of CO2 can be formed by the complete combustion of a 14.7-gram sample of C2H6 that is 92.4% pure.
To determine the grams of CO2 formed by the complete combustion of C2H6, we need to follow a few steps:
1. Calculate the molar mass of C2H6 (ethane):
- The molar mass of carbon (C) is 12.01 g/mol.
- The molar mass of hydrogen (H) is 1.01 g/mol.
- Multiply the molar mass of carbon by 2 since there are two atoms of carbon in C2H6.
- Multiply the molar mass of hydrogen by 6 since there are six atoms of hydrogen in C2H6.
- Add the results to find the molar mass of C2H6.
2. Calculate the number of moles of C2H6 in the 14.7 g sample:
- Divide the mass (14.7 g) by the molar mass of C2H6 to get the number of moles.
3. Since ethane (C2H6) combusts completely to produce CO2, every mole of C2H6 reacts to form an equal number of moles of CO2.
4. Determine the percentage purity:
- Multiply the number of moles of C2H6 (from step 2) by the purity percentage (92.4%) to calculate the number of moles of pure C2H6.
5. Calculate the number of moles of CO2 formed:
- Since the number of moles of CO2 is equal to the number of moles of pure C2H6, the value from step 4 is the number of moles of CO2.
6. Convert the number of moles of CO2 to grams:
- Multiply the number of moles of CO2 by the molar mass of CO2.
- The molar mass of carbon dioxide (CO2) is 44.01 g/mol.
Let's go through the calculations:
1. Molar mass of C2H6:
- Molar mass of carbon (C) = 12.01 g/mol.
- Molar mass of hydrogen (H) = 1.01 g/mol.
- Molar mass of C2H6 = (2 * molar mass of carbon) + (6 * molar mass of hydrogen)
= (2 * 12.01 g/mol) + (6 * 1.01 g/mol)
= 24.02 g/mol + 6.06 g/mol
= 30.08 g/mol
2. Moles of C2H6 in the 14.7 g sample:
- Moles of C2H6 = mass / molar mass
= 14.7 g / 30.08 g/mol
≈ 0.4886 mol
3. Moles of pure C2H6:
- Moles of pure C2H6 = moles of C2H6 * purity
= 0.4886 mol * 0.924
≈ 0.4516 mol
4. Moles of CO2 formed:
- Moles of CO2 = moles of pure C2H6
= 0.4516 mol
5. Grams of CO2 formed:
- Grams of CO2 = moles of CO2 * molar mass of CO2
= 0.4516 mol * 44.01 g/mol
≈ 19.86 g
Therefore, approximately 19.86 grams of CO2 will be formed by the complete combustion of the 14.7 grams sample of C2H6.