Question

Question #ee1e7

Answer 1

`"3 moles X"`

Explanation:

All you have to do here is use the molarities and the volumes of the two solutions to figure out how many moles of each reactant were needed for a complete reaction.

For substance `"X"`, you have

`20 color(red)(cancel(color(black)("cm"^3))) * (1 color(red)(cancel(color(black)("dm"^3))))/(10^3color(red)(cancel(color(black)("cm"^3)))) * "1.5 moles X"/(1color(red)(cancel(color(black)("dm"^3)))) = "0.03 moles X"`

For substance `"Y"`, you have

`10 color(red)(cancel(color(black)("cm"^3))) * (1 color(red)(cancel(color(black)("dm"^3))))/(10^3color(red)(cancel(color(black)("cm"^3)))) * "1 mole Y"/(1color(red)(cancel(color(black)("dm"^3)))) = "0.01 moles Y"`

You can thus say that the two reactants will react in a `3:1` mole ratio, since

`"0.03 moles X"/"0.01 moles Y" = (3 * color(red)(cancel(color(black)(10^(2))))color(white)(.)"moles X")/(1 * color(red)(cancel(color(black)(10^(2))))color(white)(.)"moles Y") = "3 moles X"/"1 mole Y"`

The balanced chemical equation that will describe your reaction can be written as

`3"X"_ ((aq)) + "Y"_ ((aq)) -> "products"`

Therefore, you can say that `1` mole of `"Y"` will be completely consumed by `3` moles of `"X"`.