What is the difference between vapour and gas? Vapor implies the existence of a condensed phase that is the source or destination of the gas, or with which the gas may be in equilibrium; while gas does not make such an assumption
evaporation - What is the difference between smell odor and vapor . . . 1 What is the difference between "smell odor" and "vapor" of a substance? It is assumed that the vapor of a given compound element is the gas phase of the same pure compound element By condensing the vapor, you can obtain the same stuff in liquid or solid form Smell on the other hand is a human animal perception
General rules for deciding volatility - Chemistry Stack Exchange Volatility is directly related to a substance's vapor pressure At a given temperature, a substance with higher vapor pressure vaporizes more readily than a substance with a lower vapor pressure (Taken from Wikipedia) But this doesn't seem to work--I recall that methanol is less volatile than ethanol I think you have got this wrong
thermodynamics - Why do we have water vapor at room temperature and . . . 1 Think of molecules of water liquid escaping into vapor, and molecules of water vapor condensing into liquid Both processes occur simultaneously, and an equilibrium is reached in a closed system The molecules in vapor form create a specific vapor pressure at a given temperature, as explained by the kinetic theory of gases
How to calculate the vapour density of a mixture? Was it safe to assume that the amount of substance of mixture equals that of the amount of substance of both the gases? Amount of substance is additive, just like mass You have to be careful with volume, though So yes, it is safe to make that assumption I have to figure out the vapour density of the mixture I'm not sure you are starting with a safe question, i e if the vapour density
thermodynamics - How does water sublimate at normal atmospheric . . . The lyophilizer uses the latter approach, constantly pumping the gas phase out so that the partial pressure of water vapor (which in a closed vacuum system rapidly becomes equal to total pressure because other gases are not replenished) remains below the equilibrium vapor pressure at the temperature of the sample chamber
Why does the vapour pressure not depend on the surface area and volume . . . I think that you forget about molecules re-entering the liquid from the vapour Eventually the vapour will come into equilibrium with its liquid and so the rate of leaving the liquid and the rate of colliding with the liquid surface and so re-entering, become equal When this happens the vapour pressure becomes constant