Why are you able to use the ideal gas equation for a volatile liquid to determine its relative molecular mass? Surely because it's still a liquid the forces between the particles are too high for the ideal gas equation to be used? Please explain this thoroughly, thanks!
Why are you able to use the ideal gas equation for a volatile liquid to determine its relative molecular mass? Surely because it's still a liquid the forces between the particles are too high for the ideal gas equation to be used? Please explain this thoroughly, thanks!
Why are you able to use the ideal gas equation for a volatile liquid to determine its relative molecular mass? Surely because it's still a liquid the forces between the particles are too high for the ideal gas equation to be used? Please explain this thoroughly, thanks!
I have a feeling it's something to do with the fact that it's volatile. That means it easily evaporates at room temperature...into a gas.
But in the AQA Specification it states 'Students could be asked to find the Mr of a volatile liquid.' under sub section 3.1.2.3. Are you certain it's only for gases?
But in the AQA Specification it states 'Students could be asked to find the Mr of a volatile liquid.' under sub section 3.1.2.3. Are you certain it's only for gases?
Logic would say yes
I'm sure they'll give you like the number of moles or a concentration and a volume or something
I'm sure they'll give you like the number of moles or a concentration and a volume or something
Hopefully, I may be acting paranoid but I don't want to mess up on a simple question like this if it comes up in the exam. I looked up volatile liquids and they are gases at room temperature so I think I've got it now.