Question #3331e
1 Answer
See explanation.
Explanation:
One cannot possibly answer this question without a balanced chemical equation to go by.
The general idea is that the stoichiometric coefficients present in a balanced chemical equation tell you the numbers of moles that take part in the reaction for the reactants and the products.
Take, for example, this balanced chemical equation
#"C"_ ((s)) + "O"_ (2(g)) -> "CO"_ (2(g))#
Here
Similarly, you have a
In your case, this would mean
#23 color(red)(cancel(color(black)("moles O"_2))) * "1 mole CO"_2/(1color(red)(cancel(color(black)("moles O"_2)))) = "23 moles CO"_2#
Another example would be
#"CH"_ (4(g)) + color(blue)(2)"O"_ (2(g)) -> "CO"_ (2(g)) + 2"H"_ 2"O"_ ((l))#
This time, you have a
In your case, this would mean
#23 color(red)(cancel(color(black)("moles O"_2))) * "1 mole CO"_2/(color(blue)(2)color(red)(cancel(color(black)("moles O"_2)))) = 23/2color(white)(.)"moles CO"_2#
So, make sure that you're working with a balanced chemical equation. Look at the stoichiometric coefficients for
The ratio that exists between these coefficients will give you the mole ratio that exists between the two chemical species.
Finally, set up the mole ratio as a conversion factor and calculate the number of moles of carbon dioxide produced by