Question

Given, .... `CH_4(g) + 2O_2(g) rarr CO_2(g) + 2H_2O(l) + 213*"kcal"` ...What energy will result if a `0.350*mol` quantity of dioxygen gas combusts with STOICHIOMETRIC methane?

Answer 1

You gots.....

`CH_4(g) + 2O_2(g) rarr CO_2(g) + 2H_2O(l) + 213*"kcal"`

Explanation:

And another way we could write this is as:

`CH_4(g) + 2O_2(g) rarr CO_2(g) + 2H_2O(l);DeltaH^@ =-213*kcal*mol^-1`

And the negative sign indicates an exotherm, `213*kcal` is generated PER MOLE of reaction as written.

Here were gots `0.350*mol` dioxygen gas, that is assumed to combust a `0.175*mol` quantity of methane according to the given reaction. We must assume this stoichiometry.

And so energy released is given by the product....

`0.175*molxx-213*kcal*mol^-1=-37.3*kcal`

How many moles of carbon dioxide and water will result....?