When butane undergoes complete combustion , the products are CO2 and H2O

C4H10(g) + O2(g)-> CO2(g) + H2O(g)
What is the value of the coefficient for oxygen when this equation is balanced

it should be 2C4HO + 8O2 - > 8CO2 + H20

Try this instead.

2C4H10 + 13O2 ==> 8CO2 + 10H2O

No its wrong

To balance the equation, you need to ensure that the number of each type of atom is the same on both sides of the reaction arrow. Here's how you can balance the equation:

1. Start by counting the number of carbon atoms on each side:
On the left-hand side: 1 carbon atom (C4H10)
On the right-hand side: 1 carbon atom (CO2)

2. Next, count the number of hydrogen atoms on each side:
On the left-hand side: 10 hydrogen atoms (C4H10)
On the right-hand side: 2 hydrogen atoms (H2O)

3. Finally, count the number of oxygen atoms:
On the left-hand side: 2 oxygen atoms (O2)
On the right-hand side: 2 oxygen atoms in CO2 and 1 oxygen atom in H2O, totaling 3 oxygen atoms.

To balance the equation, you need to adjust the coefficient for oxygen on the left-hand side (O2). Since there are already 2 oxygen atoms in O2 on the left side, you need to add another oxygen molecule (O2) to obtain a total of 4 oxygen atoms.

The balanced equation becomes:
C4H10(g) + 2 O2(g) -> 4 CO2(g) + 5 H2O(g)

Therefore, the coefficient for oxygen is 2.