Question

How many moles of O2 are required for the complete combustion of 0.6 mol of C4H8O?

Answer 1

For the complete combustion of 0.6 mol of
`C_4H_8O`, 3.6 moles of
`O_2` are required, as determined by the balanced chemical reaction.

The question asks how many moles of
`O_2` are required for the complete combustion of 0.6 mol of
`C_4H_8O`. To answer this, we first need the balanced chemical equation for the combustion of
`C_4H_8O`:

`C_4H_8O` +
`O_2` →
`CO_2` +
`H_2O`

However, the equation provided is unbalanced. Balancing the chemical equation:

`C_4H_8O` + 6
`O_2` → 4
`CO_2` + 4
`H_2O`

This means that for every 1 mol of
`C_4H_8O`, 6 mol of
`O_2` are required. Therefore, for the combustion of 0.6 mol of
`C_4H_8O`, we need:

0.6 mol
`C_4H_8O` × (6 mol
`O_2` / 1 mol
`C_4H_8O`) = 3.6 mol
`O_2`

Thus, 3.6 moles of
`O_2` are required for the complete combustion of 0.6 moles of
`C_4H_8O`.