Question

(5 pts) The following reaction was carried out with 3 moles of \( \mathrm{N}_{2} \) and 8 moles of \( \mathrm{H}_{2} \). Which was the limiting reactant? (When the stoichiometric coefficients are not 1 , the numbers of moles of each reactant must be divided by the coefficient for that reactant before comparison.) \[ \mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3} \] 

          (5 pts) The following reaction was carried out with 3 moles of \( \mathrm{N}_{2} \) and 8 moles of \( \mathrm{H}_{2} \). Which was the limiting reactant? (When the stoichiometric coefficients are not 1 , the numbers of moles of each reactant must be divided by the coefficient for that reactant before comparison.)
\[
\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3}
\]
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(5 pts) The following reaction was carried out with 3 moles of N2 and 8 moles of H2. Which was the limiting reactant? (When the stoichiometric coefficients are not 1 , the numbers of moles of each reactant must be divided by the coefficient for that reactant before comparison.) N2+3 H2→ 2 NH3

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Introductory Chemistry
Introductory Chemistry
Nivaldo J. Tro 5th Edition
Chapter 8
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Transcript

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00:02 All right, so for each of these problems, we're going to be solving for an unknown amount of moles of different compounds using stoichiometry.
00:10 I'm going to do three different methods of answering the same type of problem.
00:19 So at the end of the video, for your other problems, just choose the way that you like the best.
00:24 Okay, i'm going to start with the traditional railroad track method.
00:30 So the question is how many moles of h2? identify my own known.
00:35 How many moles of h2 will completely react with one mole of n2? and so my given is going to go in the top left of my railroad tracks.
00:52 So one mole of n2.
00:58 Okay? and then i can use the coefficients for each of my compounds, to figure out my conversion method.
01:08 So because i'm solving for moles of h2, i don't have to convert to grams or anything like that.
01:15 So the units that i started with must end up on the bottom.
01:19 So i put them on the bottom.
01:21 And then on the top, i can go directly to moles of h2.
01:29 So on the top, i have three moles of h2.
01:33 I got that number from right here, the coefficient.
01:36 For every three moles of h2 i have, i have one mole of n2.
01:41 If there's no number in front, then we assume it's one.
01:46 So then my units for moles of n2 cancel.
01:50 I have it on top and bottom.
01:52 One and one cancel, also one and one divided by one.
01:56 I mean one divided by one is one.
01:59 So i am left with three moles of h2, which is my answer.
02:12 Okay.
02:17 So the second time, so for the next problem, i'm going to go ahead and do that it's the same type of problem.
02:23 I'm solving for the number of moles.
02:25 I've got to convert from one compound to another.
02:28 This time i'm going to use something called a proportion method.
02:33 I'm just comparing the amount for one compound to another compound.
02:41 And so i'm going to still read my problem, so how many moles of n2 are needed to produce 0 .60 moles of ammonia.
02:52 Okay, n2, by the way, is nitrogen.
02:57 So for this one, i'm going to go out and mark my reaction.
03:02 So i am solving for the moles of n2.
03:07 I know that i'm starting with 0 .60 moles of ammonia.
03:14 So notice i put my units.
03:16 Okay, so whatever came out of the question, i put that on top.
03:24 On bottom, i'm going to write down the conversion factors.
03:28 So for n2, i have one mole of n2.
03:33 That's the coefficient.
03:36 Okay, for nh3, i have two moles of nh3.
03:40 So i want you to look at your units.
03:42 The units on the top should match the units on the bottom, and they do.
03:47 So i don't need to convert anything here.
03:50 So now i just set this up.
03:53 So i have question mark moles of n2.
03:58 And then i have one mole of n2 for every reaction...
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