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Boyle's and Charles' laws both assume that gases behave in an ideal way. What does that mean? A.) that gases behave according to Gay-Lussac's laws B.) that gases behave according to the combined gas laws C.) that gases behave according to the kinetic-molecular theory D.) that gases behave according to the laws of phase change and energy transfer
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1) Gay Lussac's law assumes gas behaves ideally so that equal volumes of different gases at the same pressure and temperature contain the same number of molecules. And that gases that undergo reaction do so in simple integral proportions. ideal gas assumptions are, by the way, 1) gas molecules have no volume, 2) no intermolecular forces, and 3) collisions are elastic - ie kinetic energy is conserved.... 2) given P1V1 = n1 R T1 and P2V2 = n1 R T2 if we assume P1 = P2 and T1 = T2, and R is a constant, then P1/(R T1) = n1/ V1 and P2/(R T2) = n1/ V2 or n1/ V1 = n2 / V2 and V2 / V1 = n2 / n 1
What factors cause real gases to behave in a non-ideal way?
The forces of attraction and the volume of the molecules (as opposed to the volume of the container the gas is in). These are represented respectively by the variables a and b in the van der Waals equation, a variation of the ideal gas law. http://hyperphysics.phy-astr.gsu.edu/Hbase/Kinetic/waal.html Van der Waals equation can be seen here.
Helium has only two electrons. Why does it behave as a noble gas?
In the first electron shell, it can only contain 2 electrons. Therefore, it has a full valence (outermost) shell.