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

Combustion Analysis

General Chemistry

3. Chemical Reactions

Combustion Analysis

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Multiple Choice

When 0.112 g of heptene, C7H14, is burned in a bomb calorimeter, the temperature rises by 4.99 °C. The heat capacity of the calorimeter is 2.46 kJ/°C. Calculate the combustion energy (ΔE) for heptene, C7H14, in kJ/g. Express your answer in kJ/g.

-98.3 kJ/g

-115.2 kJ/g

-120.7 kJ/g

-109.5 kJ/g

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Verified step by step guidance

Step 1: Understand the problem. We need to calculate the combustion energy (ΔE) for heptene, C7H14, in kJ/g using the data provided from the bomb calorimeter experiment.

Step 2: Use the formula for heat transfer in a calorimeter: \( q = C \times \Delta T \), where \( q \) is the heat absorbed or released, \( C \) is the heat capacity of the calorimeter, and \( \Delta T \) is the change in temperature.

Step 3: Substitute the given values into the formula: \( q = 2.46 \text{ kJ/°C} \times 4.99 \text{ °C} \). This will give you the total heat released during the combustion of heptene.

Step 4: Calculate the combustion energy per gram of heptene. Use the formula \( \Delta E = \frac{q}{ ext{mass of heptene}} \). Substitute \( q \) from Step 3 and the mass of heptene (0.112 g) into the formula.

Step 5: Express the result in kJ/g. This will give you the combustion energy of heptene in kJ/g, which you can compare to the provided options to identify the correct answer.