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?

1 Answer
Oct 19, 2017

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....?