Question

How many molecules of water will be produced if 52.6 g of methane are burned?

6.6x1023
none of these
3.96x1024
1.32x1024

Answer 1

Answer:
`3.96 * 10^(24)`

Step-by-step explanation:

The balanced equation for the combustion of methane is
`\text{CH}_4+2\text{O}_2 \longrightarrow \text{CO}_2+2\text{H}_2\text{O}`.

The molar mass of methane is 16 g/mol, so 52.6 g of methane is equal to 3.2875 moles.

For every one mole of methane comsumed, we know that 2 moles of water are produced. Therefore, there are
`6.575` moles of water.

Avogadro's number states that there are
`6.022 * 10^(23)` molecules of water per mole. Therefore, there is a total of
`6.575 * (6.022 * 10^(23))=3.96 * 10^(24)` molecules of water.