One mole of neon gas is heated from 300. K to 420. K at...

Name: Problem 69, Chapter 12: College Physics
Uploaded: 2019-11-23T18:35:30-08:00
Duration: 2 min 24 s
Channel: Averell Hause
Description: One mole of neon gas is heated from 300. K to 420. K at constant pressure. Calculate (a) the energy Q transferred to the gas, (b) the change in the internal energy of the gas, and (c) the work done on the gas. Note that neon has a molar specific heat of c 5 20.79 J/mol?K for a constant-pressure process.

One mole of neon gas is heated from 300. K to 420. K at constant pressure. Calculate (a) the energy Q transferred to the gas, (b) the change in the internal energy of the gas, and (c) the work done on the gas. Note that neon has a molar specific heat of c 5 20.79 J/mol?K for a constant-pressure process.

Key Concepts

Molar Specific Heat Capacity

Molar specific heat capacity is the amount of heat required to raise the temperature of one mole of a substance by one degree Kelvin. For processes at constant pressure, this value is used to calculate the heat transferred to the gas when its temperature changes.

Constant Pressure Process

A constant pressure process implies that the pressure remains unchanged during the heating or cooling of the system. In thermodynamics, this condition affects the work done by the gas, which is given by the product of pressure and the change in volume.

Work Done by a Gas

In a thermodynamic process, the work performed by or on a gas is calculated by the area under the pressure-volume curve. For a constant pressure process, the work done by the gas is directly proportional to the change in volume and can be calculated as the product of constant pressure and the change in volume.

Internal Energy

Internal energy refers to the total energy contained within the system, including kinetic and potential energies at the microscopic scale. For an ideal gas, the internal energy is solely a function of temperature, and its change can be computed by utilizing the specific heat capacity at constant volume.

First Law of Thermodynamics

The First Law of Thermodynamics is the principle of energy conservation, stating that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system on its surroundings. This law provides the foundation for understanding energy transfers in thermodynamic processes.

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