solid C₄H₁₀O is burned with oxygen gas to produce gaseous carbon dioxide and water vapor
yes, this is true
now just google "C4H10O + O2"
Well, well, well, it looks like our good ol' friend C₄H₁₀O decided to have a fiery adventure with some oxygen gas! They must have been feeling a little hot under the collar. Anyway, when these two got together, they created some gaseous carbon dioxide and water vapor. Talk about a dynamic duo, am I right?
But hey, speaking of burning things, did you hear about the fire at the circus? It was in-tents!
To balance the combustion reaction of C₄H₁₀O with oxygen gas to produce carbon dioxide (CO₂) and water vapor (H₂O), follow these steps:
Step 1: Write the unbalanced equation:
C₄H₁₀O + O₂ → CO₂ + H₂O
Step 2: Count the number of carbon (C) atoms on both sides of the equation. In this case, there are 4 carbon atoms on the left side (C₄H₁₀O) and 1 carbon atom on the right side (CO₂).
To balance the carbon atoms, place a coefficient of 4 in front of CO₂:
C₄H₁₀O + O₂ → 4CO₂ + H₂O
Step 3: Count the number of hydrogen (H) atoms on both sides of the equation. There are 10 hydrogen atoms on the left side (C₄H₁₀O) and 2 hydrogen atoms on the right side (H₂O).
To balance the hydrogen atoms, place a coefficient of 5 in front of H₂O:
C₄H₁₀O + O₂ → 4CO₂ + 5H₂O
Step 4: Count the number of oxygen (O) atoms on both sides of the equation. On the left side, there are 2 oxygen atoms from O₂ and 10 oxygen atoms from C₄H₁₀O, totaling 12 oxygen atoms. On the right side, there are 8 oxygen atoms from 4CO₂ and 10 oxygen atoms from 5H₂O, totaling 18 oxygen atoms.
To balance the oxygen atoms, place a coefficient of 6.5 (or 13/2) in front of O₂:
C₄H₁₀O + 6.5O₂ → 4CO₂ + 5H₂O
Since it's not possible to have a fraction as a coefficient, we can multiply the entire equation by 2 to eliminate the fraction:
2C₄H₁₀O + 13O₂ → 8CO₂ + 10H₂O
Therefore, the balanced equation is:
2C₄H₁₀O + 13O₂ → 8CO₂ + 10H₂O
To balance the chemical equation for the combustion of solid C₄H₁₀O (a hydrocarbon) with oxygen gas (O₂) to produce gaseous carbon dioxide (CO₂) and water vapor (H₂O), we follow these steps:
Step 1: Write the chemical formula for the reactants and products:
C₄H₁₀O + O₂ → CO₂ + H₂O
Step 2: Count the number of atoms for each element on both sides of the equation:
Reactants: C: 4 atoms, H: 10 atoms, O: 1 atom
Products: C: 1 atom, H: 2 atoms, O: 3 atoms
Step 3: Balance the carbon (C) atoms by placing a coefficient in front of CO₂:
C₄H₁₀O + O₂ → 4CO₂ + H₂O
Step 4: Balance the hydrogen (H) atoms by placing a coefficient in front of H₂O:
C₄H₁₀O + O₂ → 4CO₂ + 5H₂O
Step 5: Balance the oxygen (O) atoms by placing a coefficient in front of O₂:
C₄H₁₀O + 6.5O₂ → 4CO₂ + 5H₂O
Since coefficients must be whole numbers, the coefficients are usually multiplied by the same factor to get rid of the decimal. In this case, we would multiply all the coefficients by 2 to simplify the equation:
2C₄H₁₀O + 13O₂ → 8CO₂ + 10H₂O
Therefore, the balanced equation for the combustion of solid C₄H₁₀O with oxygen gas is:
2C₄H₁₀O + 13O₂ → 8CO₂ + 10H₂O