Individual samples of O2, N2, and He are present in a 1.25 L, 2.40L, and 6.10L vessel respectively. Each exerts a pressure of 1.50 atm. If all three gases are forced into the same 1.00 L container with no change in temperature, what will be the resulting pressure? What is the partial pressure of O2, N2, and He in the mixture?

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A: Repeated trials means measurement of same  data repeatedly.

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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.