If 35.8 g of CH4 and 75.5 g of S react, how many grams of H2 S are produced? (9.2,9.3,9.4) CH

If 35.8 g of CH4 and 75.5 g of S react, how many grams of...

If $35.8 \mathrm{~g}$ of $\mathrm{CH}_{4}$ and $75.5 \mathrm{~g}$ of $\mathrm{S}$ react, how many grams of $\mathrm{H}_{2} \mathrm{~S}$ are produced? $(9.2,9.3,9.4)$
$$
\mathrm{CH}_{4}(g)+4 \mathrm{~S}(g) \longrightarrow \mathrm{CS}_{2}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g)
$$

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Key Concepts

Stoichiometry

Stoichiometry is the method of calculating the relative quantities of reactants and products in a chemical reaction based on the balanced chemical equation. It involves converting mass to moles, applying mole ratios, and converting back to mass if needed.

Limiting Reactant

The limiting reactant is the reactant that is completely consumed first, dictating the maximum amount of product that can be formed in a chemical reaction. Identifying it requires comparing the mole ratios of the available reactants.

Balanced Chemical Equation

A balanced chemical equation displays the relative amounts of reactants and products with stoichiometric coefficients that preserve the number of atoms for each element. This is essential for accurately relating the quantities involved in a reaction.

Molar Mass

Molar mass, the mass of one mole of a substance, is used to convert between mass and the number of moles. It is a fundamental concept in quantitative chemical analysis.

Transcript

00:02 Here we're given a reaction between aluminum and hcl, forming hydrogen gas, and we're asked how many grams of hydrogen gas are produced.

00:10 First, we need to balance the equation.

00:12 We notice here we have one chlorine and three chlorines.

00:16 I'm going to actually use a multiplier of six here, just to keep things even in the end, and that means we need a two here that balances the fluorines, and we need two to balance the aluminum.

00:32 And now over here we have six hydrogens, so we need three here.

00:37 So that's balanced now.

00:39 We also always want to be working in moles.

00:41 So let's turn this 1 .84 grams into moles.

00:45 And the molecular weight of aluminum is 26 .98 grams per mole.

00:55 And we want to remember that molecular weight is mass divided by number of moles.

01:05 So number of moles is going to be mass divided by molecular weight, which is going to be our 1 .84 grams divided by 26 .98 grams per mole.

01:25 And our grams cancel, moles come to the top.

01:31 And that gives us 6 .820.

01:39 Times 10 to the minus 2 moles of aluminum.

01:45 Now we want to know how many moles of hcl do we have to work with.

01:50 So here we're going to use the expression since we're given concentrations for solutions.