Vapour pressure is the pressure exerted by vapour molecules over a liquid surface.
The vapour pressure is a property
a) inter molecular forces: higher the inter molecular forces lower the vapour pressure, In this case we have taken same liquid (milk) hence in all case the inter molecular forces will be same.
b) Temperature: higher the temperature higher the kinetic energy of molecules and more the tendency of liquid molecules to convert to vapor phase.
The vapor pressure will be independent of the container being closes or open.
Thus vapor pressure will be high in Bowl B which is uncovered, and the milk is warmer than room temperature, as it has higher temperature than all other bowl of milk.
Answer:
One element takes the place of another in a compound
Explanation:
a p e x - just did the test
Moving from Ethanol through Propanol to Butanol the physical properties like boiling points, surface tension and viscosity increases because of the increases in intermolecular interactions between the molecules of given compounds.
Explanation:
Ethanol, propanol and butanol all have hydroxyl groups in common, means all have hydrogen bond intractions between their molecules. So, taking the hydrogen bonding interaction constant we are left with only the difference in the number of carbon atoms.
Butanol has the greatest physical properties than other two because it has four carbon atom chain. So, as we know the London Dispersion forces or Van der Waal forces increases with increase in molecular size and chain length of hydrocarbon.
Therefore, the strength of London forces is greater in butanol than other two while ethanol has the smallest chain comparatively hence, lowest physical properties.
Let's hope she didn't watch it without me or i will never be speaking to her again :))
