Consider the reaction MnO2+4 HCl ⟶MnCl2+Cl2+2 H2 O If 0.86 mole of MnO2 and 48.2 g of HCl react

Consider the reaction MnO2+4 HCl ⟶MnCl2+Cl2+2 H2 O If 0.86...

Consider the reaction $$\mathrm{MnO}_{2}+4 \mathrm{HCl} \longrightarrow \mathrm{MnCl}_{2}+\mathrm{Cl}_{2}+2 \mathrm{H}_{2} \mathrm{O} $$If 0.86 mole of $\mathrm{MnO}_{2}$ and $48.2 \mathrm{~g}$ of $\mathrm{HCl}$ react, which reactant will be used up first? How many grams of $\mathrm{Cl}_{2}$ will be produced?

Key Concepts

Limiting Reactant

The limiting reactant is the reactant that is completely consumed first during a chemical reaction, thereby determining the maximum amount of product that can be formed. Identifying the limiting reactant is essential for accurately predicting the yields of products.

Mole Concept

The mole concept provides a bridge between the atomic scale and macroscopic amounts of material by defining a mole as a specific number of particles (Avogadro's number). It is critical in converting between the mass of substances and the number of moles for use in stoichiometric calculations.

Chemical Reaction Stoichiometry

Chemical reaction stoichiometry involves using the balanced chemical equation to determine the relationships between the amounts of reactants and products. It provides the mole ratios that allow one to calculate how many moles of each substance will react or be produced under given conditions.

Mass-to-Mole Conversion

Mass-to-mole conversion is the process of using the molar mass of a substance to convert a given mass into moles. This conversion is fundamental in reactions, as it allows the quantitative use of the balanced equation’s ratios when analyzing the amounts of reactants and products.

Transcript

00:01 So for this problem, we have a reaction that includes mno2 as well as hydrochloric acid.

00:06 And the first thing that we want to find is what is the limiting reactant, or which reactant will be used at first.

00:12 So we know that we are dealing with this chemical equation.

00:27 And we know that we have some initial quantities for both of our reactants.

00:31 Well, for mno2, it is 0 .86 mole.

00:39 And then for the hydrochloric acid, it's 48 .2 grams.

00:48 So the first thing that we're going to do is we're going to use the mole -to -mole ratio of mno2 to hcl to find how many moles of hcl are required in this reaction.

00:59 So we know that we have 0 .86 moles of mn -o -2.

01:06 And this calculation is just going to basically be how many moles of hcl are required? required to use all of the mno2.

01:12 So we know that the multiple ratio is 4 to 1, as we can see from the coefficients.

01:22 And when you perform this calculation, we'll see that 3 .44 moles of hcl are required to react with all of the mno2.

01:33 So now we want to find how many moles of hcl do we actually have, and we can do that with the grams that we're given.

01:40 But first, we want to find the molar mass of hcl.

01:43 Well, for hcl, we know that we are dealing with one hydrogen, which is 1 .08 grams per mole.

01:54 And for cl, we have 35 .45.

01:59 So the molar mass, when you round everything together, is 36 .46 grams per mole.

02:07 So now that we have that, we can do our conversions.

02:09 So we have 48 .2 grams of hcl...

Please give Ace some feedback