Butane gas, C4H10(g), is commonly used as a fuel in barbeque gas cylinders. Write a balanced chemical equation for the combustion of butane gas
2C4H10 + 13O2 ==> 8CO2 + 10H2O
To write a balanced chemical equation for the combustion of butane gas, we need to determine the reactants and the products involved.
The reactant in this case is butane gas, which is C4H10. The combustion of butane gas involves its reaction with oxygen gas (O2) from the air. The products of this reaction are carbon dioxide (CO2) gas and water (H2O) vapor.
Now, let's write the balanced chemical equation:
C4H10(g) + O2(g) → CO2(g) + H2O(g)
To balance the equation, we need to ensure that the same number of each type of atom is present on both sides. First, let's balance the carbon (C) atoms:
C4H10(g) + O2(g) → 4CO2(g) + H2O(g)
Next, let's balance the hydrogen (H) atoms:
C4H10(g) + O2(g) → 4CO2(g) + 5H2O(g)
Finally, let's balance the oxygen (O) atoms:
C4H10(g) + 13/2 O2(g) → 4CO2(g) + 5H2O(g)
Note: Since the coefficient of O2 is not a whole number after balancing the carbon and hydrogen atoms, we can multiply the entire equation by 2 to eliminate the fraction:
2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)
So, the balanced chemical equation for the combustion of butane gas, C4H10(g), is 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g).