Methanol (CH4O0, which is used as a fuel in high performance racing cars, burns in the presence of )2 to form CO2 and H2O. The molar masses for all substances are given under the balanced equation.
2 Ch4O9l) + 3 O2(g)-->2 CO2(g)+ 4H2O9g)
32.0g/mol 32.g/mol 44.0g/mol 18.g/mol
To calculate the molar masses of the substances involved in the reaction, you can refer to the periodic table for the atomic masses of each element. Here's how to calculate them:
1. Methanol (CH4O):
- Carbon (C) has an atomic mass of 12.01 g/mol
- Hydrogen (H) has an atomic mass of 1.01 g/mol
- Oxygen (O) has an atomic mass of 16.00 g/mol
Now, sum up the atomic masses of each element:
Molar mass of CH4O = (1 × molar mass of C) + (4 × molar mass of H) + (1 × molar mass of O)
Molar mass of CH4O = (1 × 12.01 g/mol) + (4 × 1.01 g/mol) + (1 × 16.00 g/mol)
Molar mass of CH4O = 32.04 g/mol
2. Carbon Dioxide (CO2):
- Carbon (C) has an atomic mass of 12.01 g/mol
- Oxygen (O) has an atomic mass of 16.00 g/mol
Sum up the atomic masses of each element:
Molar mass of CO2 = (1 × molar mass of C) + (2 × molar mass of O)
Molar mass of CO2 = (1 × 12.01 g/mol) + (2 × 16.00 g/mol)
Molar mass of CO2 = 44.01 g/mol
3. Water (H2O):
- Hydrogen (H) has an atomic mass of 1.01 g/mol
- Oxygen (O) has an atomic mass of 16.00 g/mol
Sum up the atomic masses of each element:
Molar mass of H2O = (2 × molar mass of H) + (1 × molar mass of O)
Molar mass of H2O = (2 × 1.01 g/mol) + (1 × 16.00 g/mol)
Molar mass of H2O = 18.02 g/mol
Finally, the molar masses for each substance are:
- Methanol (CH4O): 32.04 g/mol
- Carbon Dioxide (CO2): 44.01 g/mol
- Water (H2O): 18.02 g/mol