Ammonia is produced by the chemical reaction of nitrogen and...

Ammonia is produced by the chemical reaction of nitrogen and hydrogen. $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$ a. How many moles of $\mathrm{H}_{2}$ are needed to react with $1.8 \mathrm{~mol}$ of $\mathrm{N}_{2}$ ? b. How many moles of $\mathrm{N}_{2}$ reacted if $0.60 \mathrm{~mol}$ of $\mathrm{NH}_{3}$ is produced? c. How many moles of $\mathrm{NH}_{3}$ are produced when $1.4 \mathrm{~mol}$ of $\mathrm{H}_{2}$ reacts?

Ammonia is produced by the chemical reaction of nitrogen and hydrogen.
$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$
a. How many moles of $\mathrm{H}_{2}$ are needed to react with $1.8 \mathrm{~mol}$ of $\mathrm{N}_{2}$ ?
b. How many moles of $\mathrm{N}_{2}$ reacted if $0.60 \mathrm{~mol}$ of $\mathrm{NH}_{3}$ is produced?
c. How many moles of $\mathrm{NH}_{3}$ are produced when $1.4 \mathrm{~mol}$ of $\mathrm{H}_{2}$ reacts?

Key Concepts

Mole Ratios

Mole ratios are derived from the coefficients in a balanced chemical equation and are used to convert between moles of different substances. They are crucial for calculating how much of one reactant is required to completely react with a given amount of another reactant or to predict the amount of product formed.

Mole Concept

The mole concept is a fundamental principle in chemistry that defines a mole as a specific number of particles (usually atoms or molecules). It provides a bridge between the atomic scale and measurable amounts of substances, enabling chemists to relate masses to the number of particles in chemical reactions.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships of the reactants and products in a chemical reaction. It allows chemists to calculate how much of each substance is needed or produced when a reaction occurs.

Balanced Chemical Equation

A balanced chemical equation accurately represents a chemical reaction by ensuring that the number of atoms of each element is equal on both sides of the equation. This is essential for determining the correct proportions or mole ratios of reactants and products.

Transcript

0:00 All right.

00:01 So this question is asking us about the production of ammonia through the reaction of nitrogen and hydrogen.

00:09 So the reaction given is hydrogen gas is reacting with hydrogen gas to form ammonia gas.

00:32 All right.

00:33 And this is a balanced equation.

00:35 And so it's asking us about the relationship between these molecules and this reaction and how many moles are needed.

00:40 Needed to react with the molecules.

00:44 And so question a is asking us, if 1 .8 moles of nitrogen is formed, how many moles of hydrogen were needed to react with all of this nitrogen? and so basically what we're going to do is we know that we start with the moles of nitrogen.

01:08 And so it's asking us, well, if i have this much nitrogen, how much hydrogen is going to be needed to react with all of this nitrogen.

01:17 And so we're going to need to find the mold to mole factor for this reaction between nitrogen and hydrogen.

01:23 Between nitrogen and hydrogen.

01:25 And so since there is no coefficient, it is assumed that this is a one in front of nitrogen.

01:31 So that would be the coefficient.

01:32 And so we're going to use this one and this three.

01:34 And since we were given nitrogen, we're going to put that on the bottom.

01:38 So in this fraction that the tops will, the moles of nitrogen will cancel out.

01:45 Because you can basically say that this is over 1.

01:47 And so since we're going to put the moles of nitrogen on the bottom, these units will cancel out.

01:56 And so it's one mole of nitrogen to three moles of hydrogen.

02:04 And i just got those numbers right from the balanced equation that was provided.

02:08 And so to solve this now, we're just going to do 1 .8 times 3, since 3 is on the top.

02:13 And we get 5 .4 moles.

02:21 Of hydrogen needed to react with 1 .8 moles of nitrogen for this chemical reaction.

02:31 All right.

02:32 And so in part b, they are asking us how many moles of nitrogen reacted if 0 .6 moles of ammonia is formed.

02:42 And so starting off, they give us that 0 .60 moles of ammonia was formed.

02:53 And they want to know how many moles of nitrogen was used in producing that 0 .6 moles...

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