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

8. Thermochemistry

Constant-Volume Calorimetry

General Chemistry

8. Thermochemistry

Constant-Volume Calorimetry

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Multiple Choice

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter. The balanced reaction is: 4 C6H5NH2(l) + 35 O2(g) → 24 CO2(g) + 14 H2O(g) + 4 N2(g). Given that the standard enthalpy of combustion for aniline is -3170 kJ/mol, what is the heat capacity of the calorimeter?

5.89 kJ/°C

6.45 kJ/°C

7.02 kJ/°C

8.15 kJ/°C

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Verified step by step guidance

Calculate the number of moles of aniline combusted using its mass and molar mass. Use the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).

Determine the total heat released during the combustion of the aniline sample using the standard enthalpy of combustion. Multiply the moles of aniline by the standard enthalpy of combustion: \( q = \text{moles} \times \Delta H_{\text{combustion}} \).

Recognize that the heat released by the combustion of aniline is absorbed by the calorimeter, causing the temperature to rise. Therefore, the heat absorbed by the calorimeter \( q_{\text{calorimeter}} \) is equal to the heat released by the reaction.

Use the formula for heat absorbed by the calorimeter: \( q_{\text{calorimeter}} = C_{\text{calorimeter}} \times \Delta T \), where \( C_{\text{calorimeter}} \) is the heat capacity of the calorimeter and \( \Delta T \) is the change in temperature.

Rearrange the formula to solve for the heat capacity of the calorimeter: \( C_{\text{calorimeter}} = \frac{q_{\text{calorimeter}}}{\Delta T} \). Substitute the values for \( q_{\text{calorimeter}} \) and \( \Delta T \) to find the heat capacity.