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

Limiting Reagent

General Chemistry

3. Chemical Reactions

Limiting Reagent

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Multiple Choice

Suppose 0.0350 g of Mg is reacted with 10.00 mL of 6 M HCl to produce aqueous magnesium chloride and hydrogen gas according to the reaction: Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g). What is the limiting reactant in this reaction?

Magnesium chloride (MgCl₂)

Hydrogen gas (H₂)

Hydrochloric acid (HCl)

Magnesium (Mg)

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Verified step by step guidance

Step 1: Begin by writing the balanced chemical equation for the reaction:

{Mg}_{(s)} + 2 {HCl}_{(aq)} \to {MgCl}_{2} (aq) + H_{2} (g)

Step 2: Calculate the moles of magnesium (Mg) using its molar mass. The molar mass of Mg is approximately 24.31 g/mol. Use the formula:

moles = \frac{mass}{molar mass}

Step 3: Calculate the moles of hydrochloric acid (HCl) using its concentration and volume. Use the formula:

moles = concentration \times volume

. Remember to convert the volume from mL to L by dividing by 1000.

Step 4: Compare the mole ratio of the reactants to the coefficients in the balanced equation. The balanced equation shows that 1 mole of Mg reacts with 2 moles of HCl. Determine which reactant is present in a smaller stoichiometric amount.

Step 5: Identify the limiting reactant as the one that will be completely consumed first based on the stoichiometric calculations. The reactant with fewer moles than required by the balanced equation is the limiting reactant.