Question #e811d
1 Answer
Explanation:
Start by writing a balanced chemical equation that describes this synthesis reaction
#"N"_ (2(g)) + color(blue)(3)"H"_ (2(g)) -> color(red)(2)"NH"_ (3(g))#
The thing to remember about balanced chemical equations is that the coefficients added in front of a chemical species represent the number of moles of said chemical species needed in order for the reaction to take place.
In this case, you need
Now, these mole ratios are true regardless of how many moles of a particular chemical species you have. In other words, you will have
#"number of moles of N"_2/"number of moles of NH"_3 = 1/color(red)(2)#
Similarly, you will also have
#"number of moles of H"_2/"number of moles of N"_2 = color(blue)(3)/1#
and
#"number of moles of H"_2/"number of moles of NH"_3 = color(blue)(3)/color(red)(2)#
In your case, you know that
#"no. of moles of N"_2 = 1/color(red)(2) * "no. of moles of NH"_3#
you can say that the reaction consumed
#"no. of moles of N"_2 = 1/color(red)(2) * "0.85 moles" = color(darkgreen)(ul(color(black)("0.43 moles N"_2)))#
The answer must be rounded to two sig figs, the number of sig figs you have for the number of moles of ammonia produced by the reaction.