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The mass of 1.00 mol of helium gas, assumed to be an ideal gas, is 4.00g. Calculate the root-mean-square (r.m.s.) speed of an atom of helium gas for a temperature of 27 oc.
Explain how the ideal gas equation can be constructed by combining Charles’s, Boyle’s, and Avogadro’s Laws, and explain how the ideal gas equation can be used to derive each of the three two-variable laws.
A gas consists of molecules of negligible volume. The molecules collide elastically with each other and the container, thus gaining or losing no energy. There are negligible forces of attraction between the molecules. The duration of an impact is much less than the time between impacts.
the gas cannot be liquified there are no interactions between molecules (except during collisions) the gas obeys the (ideal) gas law / obeys Boyles law etc. at all temperatures/pressures any two lines a gas laws may be given as a formula 2 16 (b) (i) n (= PV / RT) = 1.60 × 106 × 0.200 / (8.31 × (273 + 22))
Any equation that relates the pressure, temperature, and specific volume of a substance is called an equation of state. The simplest and best known equation of state for substances in the gas phase is the ideal-gas equation of state.
Summary of Gas Laws: The Ideal Gas Law {Boyle’s Law - V ∝1/P (at constant T & n) {Charles’ Law – V ∝T (at constant P & n) {Avogadro’s Law – V ∝n (at constant T & P) {Combine these three laws into one statement V ∝nT/P {Convert the proportionality into an equality. V = nRT/P {This provides the Ideal Gas Law. PV = nRT
R is the Molar Gas Constant, R = 8.31 J K-1 mol-1. This is called the equation of state for an ideal gas. The concept of ideal gases is used to approximate the behaviour of real gases. Real gases can become liquids at low temperatures and high pressures.
