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

The reaction between nitrogen and hydrogen to form ammonia is carried out in a flask containing 30.5 g of N2 and 8.65 g of H2. What is the theoretical yield of NH3 in grams? N2(g) + 3H2(g) → 2NH3(g)

34.0 g

25.0 g

40.0 g

28.0 g

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Verified step by step guidance

First, calculate the molar mass of N2 and H2. The molar mass of N2 is approximately 28.02 g/mol, and the molar mass of H2 is approximately 2.02 g/mol.

Next, determine the number of moles of N2 and H2 present. Use the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \). For N2, divide 30.5 g by 28.02 g/mol. For H2, divide 8.65 g by 2.02 g/mol.

Identify the limiting reactant by comparing the mole ratio from the balanced equation to the moles calculated. The balanced equation is \( \text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3 \). Calculate the required moles of H2 for the moles of N2 and vice versa.

Calculate the theoretical yield of NH3 based on the limiting reactant. Use the stoichiometry from the balanced equation: 1 mole of N2 produces 2 moles of NH3, and 3 moles of H2 produce 2 moles of NH3.

Finally, convert the moles of NH3 to grams using its molar mass (approximately 17.03 g/mol). Use the formula: \( \text{mass} = \text{moles} \times \text{molar mass} \).