What is the balanced equation of the complete combustion of 2-methylpropane?
2C4H10 + 13O2 ==> 8CO2 + 10 H2O
check my work.
Why did the 2-methylpropane go to combustion? Because it wanted to make some hot air!
But in all seriousness, the balanced equation for the complete combustion of 2-methylpropane (C4H10) is:
C4H10 + 13/2 O2 → 4 CO2 + 5 H2O
The complete combustion of 2-methylpropane (also known as isobutane) can be represented by the following balanced equation:
C4H10 + 6.5O2 -> 4CO2 + 5H2O
To determine the balanced equation for the complete combustion of 2-methylpropane (also known as isobutane), we need to understand the combustion process and the elements involved.
Step 1: Write the molecular formula of 2-methylpropane (C4H10).
Step 2: Identify the reactants and products in the combustion reaction.
Reactants:
- 2-methylpropane (C4H10)
- Oxygen (O2)
Products:
- Carbon dioxide (CO2)
- Water (H2O)
Step 3: Determine the number of carbon atoms on both sides of the equation. Since the reactant (C4H10) contains four carbon atoms, the products also need to have four carbon atoms to achieve balance.
Step 4: Balance the carbon atoms by adding coefficients in front of the carbon dioxide and water molecules.
C4H10 + O2 -> CO2 + H2O
Step 5: Determine the number of hydrogen atoms on both sides of the equation. The reactant (C4H10) contains ten hydrogen atoms, and the product (H2O) contains only two hydrogen atoms. To balance the hydrogen atoms, multiply the water molecule (H2O) by 5.
C4H10 + O2 -> CO2 + 5H2O
Step 6: Balance the oxygen atoms by adding coefficients in front of the oxygen molecules.
C4H10 + 13O2 -> 4CO2 + 5H2O
Therefore, the balanced equation for the complete combustion of 2-methylpropane (C4H10) is:
C4H10 + 13O2 -> 4CO2 + 5H2O