Question #ee1e7

1 Answer
Apr 5, 2017

Answer:

#"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"#.