Question

What mass of carbon dioxide is produced from complete combustion of a `6.85*g` mass of ethanol? What mass of dioxygen is required for the combustion?

Answer 1

We can rewrite the stoichiometric equation....

Explanation:

`H_3C-CH_2OH(l) + 3O_2(g) rarr 2CO_2(g) +3H_2O`

And thus each mole of ethanol, each `46*g` mass, required three moles of dioxygen gas, i.e. a mass of `96*g` of `O_2(g)`....and of course such reaction gives rise to a `142*g` mass of carbon dioxide and water....

In you scenario we got a molar quantity with respect to ethanol of...

`(6.85*g)/(46.07*g*mol^-1)=0.149*mol`

And so, given the stoichiometry, with respect to dioxygen we need a mass of `0.149*molxx3xx32.0*g*mol^-1=14.3*g`

And we generate a TWICE molar quantity of carbon dioxide...take that atmosphere...

`2xx0.149*molxx44.01*g*mol^-1=13.1*g` with respect to carbon dioxide....