Nitrogen and hydrogen react to form ammonia. N2(g)+3 H2(g) ⟶2 NH3(g) Determine the limiting reac

Nitrogen and hydrogen react to form ammonia. N2(g)+3 H2(g)...

Nitrogen and hydrogen react to form ammonia. $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) $$ Determine the limiting reactant in each of the following mixtures of reactants: a. $3.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $5.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$ b. $8.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $4.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$ c. $3.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $12.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$

Nitrogen and hydrogen react to form ammonia.
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)
$$
Determine the limiting reactant in each of the following mixtures of reactants:
a. $3.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $5.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$
b. $8.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $4.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$
c. $3.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $12.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$

Key Concepts

Mole Ratio Comparison

Mole ratio comparison involves relating the actual amounts of reactants provided to the stoichiometric coefficients from the balanced equation. By converting the moles of reactants using these ratios, one can determine which reactant is in deficit relative to the requirements and thus identify the limiting reactant.

Balanced Chemical Equation

A balanced chemical equation represents the chemical reaction with equal numbers of atoms for each element on both the reactant and product sides. This balance is crucial as it provides the mole ratios necessary to perform accurate stoichiometric calculations.

Limiting Reactant

The limiting reactant is the substance that is entirely consumed first in a chemical reaction, thereby preventing further reaction from occurring. It determines the maximum amount of product that can be formed and is found by comparing the available moles of each reactant to the proportions required by the reaction’s stoichiometry.

Stoichiometry

Stoichiometry involves using the quantitative relationships between reactants and products as given by a balanced chemical equation. It allows the calculation of the amounts of products formed or the reactants needed based on a known quantity of one substance in the reaction.

Transcript

00:01 We determine the limiting reagent for three different sets of reactive measurements.

00:07 So we'll begin with that first.

00:10 So i want to start off with our balanced equation.

00:14 We're going to have nitrogen combining with hormone.

00:23 And so that first one, we're going to have three moles of our nitrogen, and then we're going to have five moles of our nitrogen.

00:38 Of our hydrogate.

00:40 We need to figure out for all these different ones, which one is our limiting reagent.

00:44 So we talk about limiting reagents.

00:47 Whatever one is used up first is going to prevent that reaction from creating any more compound.

00:54 So the analogy i like to think of when i think of a limiting reagent, if i had meat, cheese, and bread to make a sandwich, once i run out of bread, i can no longer continue making sandwiches.

01:07 So this is going to be our, we need to find out which one is going to produce the least amount of product.

01:14 Because the one that produces the least amount of product is the one that is the least amount.

01:21 And it's going to be the one that limits the amount of product we could make.

01:25 The one that makes the most product of the two is going to be in excess.

01:30 So we need to find out which one is going to make the least amount of our product to determine our limiting reagent.

01:35 And then that's all the theoretical amount we can produce.

01:39 Because once that limiting reagent is used up, then our reaction stops.

01:44 We can no longer continue making product.

01:46 So that will be our answer for our theoretical yield.

01:51 So to start with, we're going to use our mole -to -mole ratios from our balanced reaction here.

01:57 So the first one, we're going to have three moles of nitrogen.

02:02 And for every one mole of my nitrogen, i get two moles of my ammonia.

02:11 And so i'm going to do the math here.

02:16 It tells me that i get six moles of product made if i use up all three moles of my nitrogen.

02:23 And then for my hydrogen, i got five moles to begin with of hydrogen...

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