One mole of a gas isobarically heated by 40 K receives an amount of heat 1.162 kJ. What is the

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One mole of a gas isobarically heated by 40 K receives an...

Key Concepts

Isobaric Process

An isobaric process is one that occurs at constant pressure. In such a process, the heat added to or removed from the system directly relates to changes in temperature through the specific heat capacity at constant pressure (Cp). Understanding isobaric processes is crucial for linking heat transfer to work done by the gas under constant pressure conditions.

Specific Heat at Constant Pressure (Cp)

The specific heat at constant pressure is the amount of heat required to raise the temperature of a substance by one unit while keeping the pressure fixed. In the context of ideal gases undergoing isobaric processes, Cp is used in the equation Q = n·Cp·?T, where Q is the heat added, n is the number of moles, and ?T is the change in temperature.

Specific Heat Ratio (?)

The specific heat ratio, denoted by ?, is the ratio of the specific heats at constant pressure and constant volume (? = Cp/Cv). This ratio is an important thermodynamic parameter that appears in various gas processes, such as adiabatic expansions and compressions, and helps in characterizing the behavior of gases under different thermodynamic conditions.

Application of the First Law of Thermodynamics to Gases

The First Law of Thermodynamics, which states 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, provides the foundation for analyzing energy changes in thermodynamic processes. In the case of isobaric processes for ideal gases, the law connects the heat added (using Cp) with the work done by the gas and the change in its internal energy.

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