(molar heat capacity at constant volume=f/2 R where f is then number of degrees of freedom) I think it should be 3/2R for monoatomic and 7/2Rfor diatomic and delta T is inversly proportional to heat capacity. Similarly for heat capacity at constant pressure (Cp=R+Cv) so diatomic will get a lower temprature than monoatomic ones so 1,3 monoatomic and 2,4 diatomicChestermiller said:
Monoatomic gases are made up of single atoms, such as helium or neon, while diatomic gases are made up of two atoms bonded together, such as oxygen or nitrogen. In thermodynamics, the main difference between these two types of gases is the number of degrees of freedom, or possible ways the molecules can move, which affects their energy and behavior.
The laws of thermodynamics apply to both monoatomic and diatomic gases, as they are fundamental principles that govern the behavior of all matter. These laws include the conservation of energy, the increase of entropy, and the impossibility of achieving absolute zero temperature.
The internal energy of a monoatomic gas is directly proportional to its temperature, according to the ideal gas law. This means that as the temperature of a monoatomic gas increases, so does its internal energy. However, for diatomic gases, the relationship is more complex due to the additional degrees of freedom.
Yes, this is possible because the internal energy of a gas is dependent on its temperature, pressure, and volume. Therefore, two gases with the same temperature and pressure can have different internal energies if their volumes are different. This is because the internal energy takes into account the potential energy of the molecules, which is affected by the volume of the gas.
The heat capacity of diatomic gases is generally higher than that of monoatomic gases. This is because diatomic gases have more degrees of freedom, which means they can store more energy in the form of heat. As a result, diatomic gases require more energy to increase their temperature compared to monoatomic gases.