Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

3. Chemical Reactions

Stoichiometry

General Chemistry

3. Chemical Reactions

Stoichiometry

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Multiple Choice

Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. The balanced chemical equation is: 4HCl(aq) + MnO2(s) → MnCl2(aq) + 2H2O(l) + Cl2(g). A sample of 33.7 g of MnO2 is added to a solution containing 48.3 g of HCl. What is the limiting reactant?

MnO2

MnCl2

HCl

Cl2

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Verified step by step guidance

First, identify the molar masses of the reactants involved. The molar mass of MnO2 is approximately 86.94 g/mol, and the molar mass of HCl is approximately 36.46 g/mol.

Calculate the number of moles of MnO2 using the formula: \( \text{moles of MnO2} = \frac{\text{mass of MnO2}}{\text{molar mass of MnO2}} \). Substitute the given mass of MnO2 (33.7 g) and its molar mass to find the moles.

Calculate the number of moles of HCl using the formula: \( \text{moles of HCl} = \frac{\text{mass of HCl}}{\text{molar mass of HCl}} \). Substitute the given mass of HCl (48.3 g) and its molar mass to find the moles.

Using the balanced chemical equation, determine the mole ratio between MnO2 and HCl. The equation shows that 4 moles of HCl react with 1 mole of MnO2.

Compare the calculated moles of each reactant to the stoichiometric ratio from the balanced equation to determine the limiting reactant. The reactant that provides fewer moles than required by the stoichiometric ratio is the limiting reactant.