Parameters such as pressure, volume and temperature are used to characterize the state of a gas of a given mass. If the state of the gas does not change, all or some of these parameters will change. If the pressure of a gas changes with a change in volume at a constant temperature, such a process is called an isothermal process. If the volume changes under the influence of temperature at constant pressure. Such a process is called an isobaric process. - Parameters such as pressure, volume and temperature are used to characterize the state of a gas of a given mass. If the state of the gas does not change, all or some of these parameters will change. If the pressure of a gas changes with a change in volume at a constant temperature, such a process is called an isothermal process. If the volume changes under the influence of temperature at constant pressure. Such a process is called an isobaric process.
- If the pressure changes under the influence of temperature in a constant volume, such a process is called an isochoric process. Before studying the equation of state of an ideal gas, we will study several gas laws that were discovered before the molecular-kinetic theory was created. Boyle-Marriott law. While studying isothermal gas processes, the English scientist Boyle (1662) and the French scientist Mariott (1667) created the following gas law: for a given mass of gas, the pressure of the gas at a constant temperature is inversely proportional to its volume. Gay-Lussac's laws: a) For a given mass of gas, its volume changes proportionally to temperature at constant pressure
Heat capacity depends on the conditions under which the body temperature changes. If the size of the body does not change, all the heat is spent on the change of internal energy. Here we are talking about the heat capacity of constant volume Cv. due to thermal expansion at a constant external pressure, mechanical work is done against external forces, and more heat is needed to heat it to a certain temperature. Therefore, the heat capacity at constant pressure Cp is always greater than Cv. For ideal gases, Cp-Cv=R, where R is the gas constant, equal to 8.32 J/(mol·K). - Heat capacity depends on the conditions under which the body temperature changes. If the size of the body does not change, all the heat is spent on the change of internal energy. Here we are talking about the heat capacity of constant volume Cv. due to thermal expansion at a constant external pressure, mechanical work is done against external forces, and more heat is needed to heat it to a certain temperature. Therefore, the heat capacity at constant pressure Cp is always greater than Cv. For ideal gases, Cp-Cv=R, where R is the gas constant, equal to 8.32 J/(mol·K).
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