### Calculation of Total Energy Required to Heat Benzene**Objective:** Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C\(_6\)H\(_6\)) from 0.00 °C to 95.0 °C.#### Given Data:- **Molar Mass of Benzene:** 78.11 g/mol- **Specific Heat Capacities:** - \( c_{s,solid} = 1.51 \, \text{J/g}^\circ\text{C} \) - \( c_{s,liquid} = 1.70 \, \text{J/g}^\circ\text{C} \) - \( c_{s,gas} = 1.05 \, \text{J/g}^\circ\text{C} \)- **Enthalpies of Phase Transitions:** - \( \Delta H_{fus} = 9.9 \, \text{kJ/mol} \) - \( \Delta H_{vap} = 33.8 \, \text{kJ/mol} \)- **Phase Transition Temperatures:** - **Melting Point (\(T_f\)):** 5.6 °C - **Boiling Point (\(T_b\)):** 80.08 °C#### Explanation:1. **Solid to Liquid Transition:** - Heating the solid benzene from 0.00 °C to 5.6 °C. - Melting the solid benzene at 5.6 °C.2. **Liquid to Gas Transition:** - Heating the liquid benzene from 5.6 °C to 80.08 °C. - Vaporizing the liquid benzene at 80.08 °C. - Heating the gaseous benzene from 80.08 °C to 95.0 °C.Calculating each step requires using the specific heat capacities for the different states of benzene, as well as the enthalpy values for the phase transitions. The sum of the energy required for each step will give us the total energy required.### Diagrams and Graphs*This section will include detailed diagrams or graphs illustrating the various phase changes and the associated temperatures. Each step's energy computation can also be depicted via individual energy

Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C&H6) from 0.00 °C to 95.0 °C molar mass: 78.11 g/mol Cs,solid = 1.51 J/g*°C Cs,liquid = 1.70 J/g*°C %3D Cs.gas = 1.05 J/g*°C AHfus = 9.9 kJ/mol AH = 33.8 kJ/mol vap Tf = 5.6°C Tp = 80.08°C

Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C&H6) from 0.00 °C to 95.0 °C molar mass: 78.11 g/mol Cs,solid = 1.51 J/g°C Cs,liquid = 1.70 J/g°C %3D Cs.gas = 1.05 J/g*°C AHfus = 9.9 kJ/mol AH = 33.8 kJ/mol vap Tf = 5.6°C Tp = 80.08°C

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

### Calculation of Total Energy Required to Heat Benzene

**Objective:** Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C\(_6\)H\(_6\)) from 0.00 °C to 95.0 °C.

#### Given Data:
- **Molar Mass of Benzene:** 78.11 g/mol
- **Specific Heat Capacities:**
- \( c_{s,solid} = 1.51 \, \text{J/g}^\circ\text{C} \)
- \( c_{s,liquid} = 1.70 \, \text{J/g}^\circ\text{C} \)
- \( c_{s,gas} = 1.05 \, \text{J/g}^\circ\text{C} \)
- **Enthalpies of Phase Transitions:**
- \( \Delta H_{fus} = 9.9 \, \text{kJ/mol} \)
- \( \Delta H_{vap} = 33.8 \, \text{kJ/mol} \)
- **Phase Transition Temperatures:**
- **Melting Point (\(T_f\)):** 5.6 °C
- **Boiling Point (\(T_b\)):** 80.08 °C

#### Explanation:

1. **Solid to Liquid Transition:**
- Heating the solid benzene from 0.00 °C to 5.6 °C.
- Melting the solid benzene at 5.6 °C.

2. **Liquid to Gas Transition:**
- Heating the liquid benzene from 5.6 °C to 80.08 °C.
- Vaporizing the liquid benzene at 80.08 °C.
- Heating the gaseous benzene from 80.08 °C to 95.0 °C.

Calculating each step requires using the specific heat capacities for the different states of benzene, as well as the enthalpy values for the phase transitions. The sum of the energy required for each step will give us the total energy required.

### Diagrams and Graphs

*This section will include detailed diagrams or graphs illustrating the various phase changes and the associated temperatures. Each step's energy computation can also be depicted via individual energy

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