An ideal gas confined to a container with a massless piston at the top. A massless wire is attacted to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 4.90 to 2.45L. When the external pressure is increased to 2.50 atm, the gas futher compresses from 2.45 to 1.96L In a seperate experiment with the same initial conditions of 2.50 atm was applied to the ideal gas, decreasing its volume from 4.90 to 1.96L in one step. If the final temperture was the same for both processes, what is the difference between q for the two step pocess and q for the one process in joules?

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Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.