# Question ee1e7

Apr 5, 2017

$\text{3 moles X}$

#### 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 $\text{X}$, 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 $\text{Y}$, 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

$\text{0.03 moles X"/"0.01 moles Y" = (3 * color(red)(cancel(color(black)(10^(2))))color(white)(.)"moles X")/(1 * color(red)(cancel(color(black)(10^(2))))color(white)(.)"moles Y") = "3 moles X"/"1 mole Y}$

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

$3 \text{X"_ ((aq)) + "Y"_ ((aq)) -> "products}$

Therefore, you can say that $1$ mole of $\text{Y}$ will be completely consumed by $3$ moles of $\text{X}$.