Question

Chlorine gas can be made in the laboratory by the reaction of hydrochloric acid and manganese(IV) oxide: $$ 4 \mathrm{HCl}(a q)+\mathrm{MnO}_{2}(s) \longrightarrow \mathrm{MnCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{Cl}_{2}(g) $$ When 1.82 mol of $\mathrm{HCl}$ reacts with excess $\mathrm{MnO}_{2},$ how many (a) moles of $\mathrm{Cl}_{2}$ and (b) grams of $\mathrm{Cl}_{2}$ form?

Name: Problem 68, Chapter 3: Chemistry: The Molecular Nature of Matter and Change
Uploaded: 2020-04-06T20:37:37-08:00
Duration: 2 min 10 s
Channel: Stephen Ho
Description: Chlorine gas can be made in the laboratory by the reaction of hydrochloric acid and manganese(IV) oxide: 4 HCl(a q)+MnO2(s) ⟶MnCl2(a q)+2 H2 O(g)+Cl2(g) When 1.82 mol of HCl reacts with excess MnO2, how many (a) moles of Cl2 and (b) grams of Cl2 form?

   Chlorine gas can be made in the laboratory by the reaction of hydrochloric acid and manganese(IV) oxide:
$$
4 \mathrm{HCl}(a q)+\mathrm{MnO}_{2}(s) \longrightarrow \mathrm{MnCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{Cl}_{2}(g)
$$
When 1.82 mol of $\mathrm{HCl}$ reacts with excess $\mathrm{MnO}_{2},$ how many (a) moles of $\mathrm{Cl}_{2}$ and (b) grams of $\mathrm{Cl}_{2}$ form?

Chemistry: The Molecular Nature of Matter and Change

Martin S.… 7th Edition

Chapter 3, Problem 68

Instant Answer

Solved by Expert Stephen Ho

04/06/2020

Step 1

This gives us a molar ratio of $\mathrm{HCl}$ to $\mathrm{Cl}_{2}$ of 4:1. Show more…

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Chlorine gas can be made in the laboratory by the reaction of hydrochloric acid and manganese(IV) oxide: $$ 4 \mathrm{HCl}(a q)+\mathrm{MnO}_{2}(s) \longrightarrow \mathrm{MnCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{Cl}_{2}(g) $$ When 1.82 mol of $\mathrm{HCl}$ reacts with excess $\mathrm{MnO}_{2},$ how many (a) moles of $\mathrm{Cl}_{2}$ and (b) grams of $\mathrm{Cl}_{2}$ form?

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Key Concepts

Balanced Chemical Equation

A balanced chemical equation represents the conservation of mass by ensuring that the number of atoms for each element is the same on both sides of the equation. It provides the mole ratios necessary for determining how much of each reactant is needed and how much product is formed.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in a chemical reaction using the mole ratios from the balanced equation. It helps in determining the number of moles of a product formed when a known amount of a reactant is used.

Molar Mass

The molar mass is the mass of one mole of a substance, expressed in grams per mole. It is used to convert the amount of substance (in moles) to its mass, which is essential for quantifying how much material is produced or required in a reaction.

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