### Transcription and Explanation:The table and text below provide thermodynamic values for water (H₂O) and methane (CH₄):| | **Water** | **Methane** ||---------------------|--------------|----------------|| **Cs, solid** | 2.01 J/g°C | Not known || **Cs, liquid** | 4.18 J/g°C | 1.64 J/g°C || **Cs, gas** | 2.09 J/g°C | 1.11 J/g°C || **ΔH vaporization** | 2,260 J/g | 255 J/g || **ΔH fusion** | 333 J/g | 34.3 J/g |#### Questions:a. Considering water, why is the enthalpy of vaporization higher than the enthalpy of fusion?b. Why is the enthalpy of vaporization much higher for water than for methane?c. Use the values in the table to determine how much heat is needed to heat 100 g of water that starts at room temperature, 21.5 °C to 115 °C. Show your work.---#### Explanation of the Table:- **Cs, solid, liquid, gas**: These are specific heat capacities of water and methane in different states. It indicates the amount of heat required to raise the temperature of a unit mass by one degree Celsius. - **ΔH vaporization**: Indicates the amount of energy needed to convert one gram of substance from liquid to gas at its boiling point. - **ΔH fusion**: Represents the energy required to convert one gram of solid into liquid at its melting point.This table can be used to understand the thermodynamic properties of water and methane, as well as to solve problems involving heating, melting, or vaporizing these substances.

The enthalpy of fusion (∆Hf) is termed as the quantity of energy that must be supplied to convert…

4) The table below contains thermodynamic values for water (H20) and for methane (CHA). Water Methane Cs, solid Cs, liquid Cs, gas AH vaporization | AH fusion 2.01 J/g°C 4.18 J/g°C 2.09 J/°C 2,260 J/g 333 J/g Not known 1.64 J/g°C 1.11 J/g°C 255 J/g 34.3 J/g a. Considering water, why is the enthalpy of vaporization higher than the enthalpy of fusion? b. Why is the enthalpy of vaporization much higher for water than for methane? c. Use the values in the table to below determine how much heat is needed to heat 100 g of water that starts at room temperature, 21.5 °C to 115 °C. Show

4) The table below contains thermodynamic values for water (H20) and for methane (CHA). Water Methane Cs, solid Cs, liquid Cs, gas AH vaporization | AH fusion 2.01 J/g°C 4.18 J/g°C 2.09 J/°C 2,260 J/g 333 J/g Not known 1.64 J/g°C 1.11 J/g°C 255 J/g 34.3 J/g a. Considering water, why is the enthalpy of vaporization higher than the enthalpy of fusion? b. Why is the enthalpy of vaporization much higher for water than for methane? c. Use the values in the table to below determine how much heat is needed to heat 100 g of water that starts at room temperature, 21.5 °C to 115 °C. Show

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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