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

Stoichiometry

GOB Chemistry

6. Chemical Reactions & Quantities

Stoichiometry

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2:59 minutes

Problem 58b

Textbook Question

Although Cu is not sufficiently active to react with acids, it can be dissolved by concentrated nitric acid, which functions as an oxidizing agent according to the following equation:
Cu(s) + 4 HNO₃(aq) → Cu(NO₃)₂(aq) + 2 NO₂(g) + 2 H₂O(l)
b. Is 35.0 g of HNO3 sufficient to dissolve 5.00 g of copper?

Verified step by step guidance

Step 1: Write down the balanced chemical equation for the reaction: Cu(s) + 4 HNO3(aq) → Cu(NO3)2(aq) + 2 NO2(g) + 2 H2O(l). This equation shows that 1 mole of Cu reacts with 4 moles of HNO3.

Step 2: Calculate the molar mass of Cu and HNO3. For Cu, the molar mass is approximately 63.55 g/mol. For HNO3, the molar mass is approximately 1.01 (H) + 14.01 (N) + 3 × 16.00 (O) = 63.01 g/mol.

Step 3: Convert the given mass of Cu (5.00 g) into moles using the formula: \( \text{moles of Cu} = \frac{\text{mass of Cu}}{\text{molar mass of Cu}} \). Substitute the values to find the moles of Cu.

Step 4: Use the stoichiometric ratio from the balanced equation to determine the moles of HNO3 required to react with the moles of Cu. The ratio is 1 mole of Cu to 4 moles of HNO3. Multiply the moles of Cu by 4 to find the moles of HNO3 needed.

Step 5: Convert the given mass of HNO3 (35.0 g) into moles using the formula: \( \text{moles of HNO3} = \frac{\text{mass of HNO3}}{\text{molar mass of HNO3}} \). Compare the moles of HNO3 available to the moles of HNO3 required to determine if 35.0 g of HNO3 is sufficient to dissolve 5.00 g of Cu.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the proportions of substances involved. In this case, stoichiometry will help us find out how much HNO3 is needed to completely react with a given mass of copper.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For this problem, we need to calculate the molar masses of copper (Cu) and nitric acid (HNO3) to convert the given masses into moles, which is essential for stoichiometric calculations.

Limiting Reactant

The limiting reactant is the substance that is completely consumed in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant in this scenario will allow us to determine if the provided amount of HNO3 is sufficient to dissolve the specified amount of copper.