Question #53b23
1 Answer
Explanation:
The idea here is that the coefficients added in the balanced chemical equation in front of each chemical species that takes part in the reaction tell you the mole ratios that exist between these chemical species.
In your case, you have
#"N"_ (2(g)) + 3"H"_ (2(g)) -> 2"NH"_ (3(g))#
As you can see, you have
#"N"_ (2(g)) -> "no coefficient = a coefficient of 1"# #3"H"_ (2(g)) -> "a coefficient of 3"# #2"NH"_ (3(g)) -> "a coefficient of 2"#
This means that the for every
Now, the problem tells you that you have
This means that the reaction will consume all the moles of hydrogen gas available and produce
#19 color(red)(cancel(color(black)("moles H"_2))) * overbrace("2 moles NH"_2/(3color(red)(cancel(color(black)("moles H"_2)))))^(color(blue)("from the balanced chemical equation")) = color(darkgreen)(ul(color(black)("13 moles NH"_3)))#
The answer is rounded to two sig figs.