Why Gases Behave Non-Ideally In High And Low Temperature
1. The reason that gases do not behave non-ideally in high and low temperature is because they don not follow the ways of the Kinetic molecular theory.
B. Vander Waals equation is applied to the ideal gas law because when the volume is increase in a gas the molecular volume causes it by subtracting the noble gas, which is the number of moles of the gas.
2. Liquids with strong intermolecular forces have a high surface tension and viscosity because the surface tension is defined as a resistance of a liquid, which is spread out increasing the surface area. That happened because of the inter molecular attraction between the molecules.
B. When increasing the temperature for the viscosity and surface tension in a liquid, it allows the molecules to move more freely loosening
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The difference between miscible and insoluble is that miscible is when two solutions are able to mix together to form one solution. When one substance is unable to dissolve into a solvent to create a solution.
B. Ideal gases have very little intermolecular interactions. When a gas is dissolved in a liquid the gas’ molecules release heat. That happens because it is harder for gases to dissolve in liquids at higher temperatures. When more heat is added to the reaction the attraction of the molecules gas decrease. 4. Dipole-dipole interactions are weaker than dipole-ion interactions because dipole-ion interactions are between dipoles and ions that are stronger than dipoles. In dipole-dipole interactions they are attracted by other dipoles molecular orientation the strength comes from the polarity of the molecules
A. Hydrogen does not have electrons covering in the nucleus making it hard to attract to un bonded electron pairs.
B. Hydrogen can only create hydrogen bonds with highly electronegative atoms.
C. Methanol shows hydrogen bonding because it contains highly electronegative oxygen allowing it to create a bond. Methane contains a hydrogen bond it does not bond because carbon is not
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