Methane undergoes slow atmospheric oxidation and produces carbonmonoxide. If `2xx10^(22)` oxygen molecules are used in such oxidation, what weight of methane is consumed?

Explanation

Slow atmospheric oxidation of methane is given by equation
`2CH_(4)+3O_(2)rarr2CO+4H_(2)O`
2 moles of `O_(2)=2 ` moles of `CH_(4)`
`3xx6.022xx106(23)O_(2)` molecules `-=`
The weight of `CH_(4)` consumed =
`(2xx16)" grams of "CH_(4)`
`2xx10^(22)O_(2)` molecules = ?
The weight of `CH_(4)` consumed `=(2xx10^(22)xx32)/(3xx6.022xx10^(23))=0.354g`