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

Magnesium

Hydrochloric acid

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Verified step by step guidance

First, calculate the moles of magnesium (Mg) using its molar mass. The molar mass of Mg is approximately 24.31 g/mol. Use the formula: \( \text{moles of Mg} = \frac{\text{mass of Mg}}{\text{molar mass of Mg}} \).

Next, calculate the moles of hydrochloric acid (HCl) using its concentration and volume. The concentration is given as 6 M, and the volume is 10.00 mL. Convert the volume to liters by dividing by 1000. Use the formula: \( \text{moles of HCl} = \text{concentration} \times \text{volume in liters} \).

Now, use the stoichiometry of the balanced chemical equation \( \text{Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)} \) to determine the mole ratio between Mg and HCl. According to the equation, 1 mole of Mg reacts with 2 moles of HCl.

Compare the calculated moles of Mg and HCl to determine the limiting reactant. The limiting reactant is the one that will be completely consumed first, based on the stoichiometric ratios.

Finally, identify the limiting reactant by comparing the available moles of each reactant to the required stoichiometric ratio. The reactant with fewer moles than required by the stoichiometry is the limiting reactant.