Methane, CH4, is the major component of natural gas. How...

Methane, $\mathrm{CH}_{4}$, is the major component of natural gas. How many moles of oxygen are needed to burn $16.5 \mathrm{~mol} \mathrm{CH}_{4} ?$ $$ \mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\ell) $$

Methane, $\mathrm{CH}_{4}$, is the major component of natural gas. How many moles of oxygen are needed to burn $16.5 \mathrm{~mol} \mathrm{CH}_{4} ?$
$$
\mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\ell)
$$

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Key Concepts

Stoichiometry

Stoichiometry is the area of chemistry that involves calculating the relationships between reactants and products in a chemical reaction. It relies on the unit 'mole' to quantify substances and uses the coefficients from balanced chemical equations to determine how much of each reactant is needed or how much product will be formed.

Mole Ratio

The mole ratio is derived from the coefficients of the reactants and products in a balanced chemical equation. It provides a proportionality relationship between substances, allowing one to calculate the required amount of one reactant (or product) given the amount of another.

Balanced Chemical Equation

A balanced chemical equation accurately represents the conservation of mass in a chemical reaction, ensuring that the number of atoms for each element is the same on both sides of the equation. The coefficients in the equation indicate the molar proportions of the reactants and products, which are essential for performing stoichiometric calculations.

Transcript

00:02 Hi there.

00:03 For problem number 43, we want to start out by identifying what we know and what we're trying to find.

00:11 So first of all, we do have a balanced equation.

00:15 We have methane gas.

00:16 I'm going to leave out the states of matter in this equation because they're not really needed for what we're doing.

00:23 Reacts with oxygen gas to produce carbon dioxide and water because this is a combustion reaction.

00:32 So carbon dioxide and two water molecules.

00:38 Both of the products are also in the gaseous state.

00:41 All right.

00:44 Actually, it has water as the liquid state, but typically in a combustion reaction, the water is also going to be gaseous.

00:51 But again, that doesn't really affect how we solve this problem.

00:54 So we have a balanced equation and we need to burn 16 .5 moles of the methane.

01:06 And we want to know how many moles of oxygen are required to do that.

01:11 So what we need to look at here are the coefficients to figure out the relationship between moles of methane and moles of oxygen.

01:21 And we see that it's a 1 to 2 ratio for every 1 mole of ch4.

01:27 And we know it's a 1 because there is not a coefficient in front of it...

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