Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

6. Chemical Reactions & Quantities

Molecular Formula

GOB Chemistry

6. Chemical Reactions & Quantities

Molecular Formula

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Multiple Choice

What is the molecular formula for the following compound?
Empirical Formula: NPCl₂ Molar Mass:347.64 g/mol

NPCl₂

N₃P₃Cl₆

N₂P₂Cl₂

N₄P₄Cl₈

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Verified step by step guidance

Understand the relationship between empirical and molecular formulas. The empirical formula represents the simplest whole-number ratio of atoms in a compound, while the molecular formula is a multiple of the empirical formula that matches the compound's molar mass.

Calculate the molar mass of the empirical formula NPCl2. Use the atomic masses: Nitrogen (N) = 14.01 g/mol, Phosphorus (P) = 30.97 g/mol, and Chlorine (Cl) = 35.45 g/mol. Add these together: 14.01 + 30.97 + 2(35.45).

Determine the factor by which the empirical formula must be multiplied to obtain the molecular formula. Divide the given molar mass of the compound (347.64 g/mol) by the molar mass of the empirical formula calculated in the previous step.

Multiply the subscripts in the empirical formula by the factor determined in the previous step to find the molecular formula. This involves multiplying each element's subscript in NPCl2 by the factor.

Verify that the calculated molecular formula matches one of the given options: N3P3Cl6, N2P2Cl2, or N4P4Cl8. Ensure that the molar mass of the calculated molecular formula is consistent with the given molar mass of 347.64 g/mol.