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

How many liters of dry chlorine gas can be obtained at 40.0°C and 787 mm Hg from the reaction of an aqueous solution containing 9.41 g of HCl with 2.01 g of KMnO4(s) according to the following equation? 2 KMnO4(s) + 16 HCl(aq) → 8 H2O(l) + 2 MnCl2(aq) + 5 Cl2(g)

3.75 L

2.50 L

5.00 L

1.25 L

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Verified step by step guidance

Step 1: Begin by identifying the balanced chemical equation for the reaction: \(2 \text{KMnO}_4(s) + 16 \text{HCl}(aq) \rightarrow 8 \text{H}_2O(l) + 2 \text{MnCl}_2(aq) + 5 \text{Cl}_2(g)\). This equation shows the stoichiometry of the reactants and products.

Step 2: Calculate the moles of \(\text{HCl}\) and \(\text{KMnO}_4\) using their molar masses. The molar mass of \(\text{HCl}\) is approximately 36.46 g/mol, and the molar mass of \(\text{KMnO}_4\) is approximately 158.04 g/mol. Use the formula \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\) for each reactant.

Step 3: Determine the limiting reactant by comparing the mole ratio from the balanced equation. The balanced equation requires 16 moles of \(\text{HCl}\) for every 2 moles of \(\text{KMnO}_4\). Calculate the moles of \(\text{Cl}_2\) produced based on the limiting reactant using the stoichiometry of the reaction.

Step 4: Use the ideal gas law \(PV = nRT\) to find the volume of \(\text{Cl}_2\) gas produced. Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. Use \(R = 0.0821 \text{ L atm/mol K}\) and convert pressure from mm Hg to atm (1 atm = 760 mm Hg).

Step 5: Solve for the volume \(V\) using the rearranged ideal gas law formula \(V = \frac{nRT}{P}\), where \(n\) is the moles of \(\text{Cl}_2\) calculated in Step 3, \(R\) is the gas constant, \(T\) is the temperature in Kelvin, and \(P\) is the pressure in atm.