@@ProfessorDaveExplains sir in our text book there’s a statement that the distance between particles of gases is 300 times greater than their diameters so thier sizes and masses do not affect their volume.I’m confused
Correct, the volume of the particles themselves is negligible under KMT. This ends up being a reasonable assumption at relatively high temperatures and relatively low pressures.
l have two gas 1 hydrogen 2 oxygen suppose l filled equal volume of both two gases in a balloon keeping temperature and pressure at constant .... here outer pressure is 1kp .....and both have same kinetic energy Now oxygen has more mass than hydrogen then oxygen should apply more pressure on container if it happens then how both two has have same volume Mr. dave please help me
Mr. dave l am not talking how they treated but l want to know exactly For a few minute only forget all the law of boyle, avagadro etc. Imagine in your mind Two balloon one with hydrogen and second with oxygen Particle of both have same kinetic energy and outer pressures is same so internal pressure must be same but oxygen have more mass than hydrogen so this balloon should have more pressure then how volume is same l want to talk face to face then you understand what's my problem is Mr. dave please do something for this problem
@@ProfessorDaveExplains Thank you for yoy reply! :) Where I am lost is, in the video, you mentioned 1 mole of gas occupies 22.4 L, textbooks mention 24 L.
Well explained by Professor Dave. These basic concepts have been presented very well. Its very easy to grasp these concepts after watching this video.
I can never get enough of your introduction and say the least your lectures. You're amazing! /Pharmacy student in Sweden
I am so glad my teacher uses your videos when teaching us.
me too
How i missed you chemistry Jesus
He knows a lot about the science talks , professor dave explains!
used to think it was 'he knows a lot about the science and stuff' not having good listening skills hurts😢
4:25 is there any reason not to just use PV=nRT / V=nRT/P for this type of problem?
you get the same answer using that rewritten formula for V, its just that multiplying by that 22.4 L volume per 1 mole in a gas is simpler
@ thanks for replying. I’ve learned a lot more since I posted this so I understand it now
Thank you ❤
In addition to the molar mass, you've got the density.
Thanks
This never made sense to me, there here gasses heavier then air and others lighter then air, how can they all have the same formula and constants?
thank you
The like to dislike ratio is undefined.
sir you have said that ... at stp .. pressure is 1 bar ... bt you are taking 1 atm . while calculating volume of gas from ideal gas equations
it's not 1 bar at stp. it's 1 atm
Sir why molar volume is same for different gases?
Because their identity is irrelevant, given the assumptions of kinetic molecular theory.
@@ProfessorDaveExplains sir in our text book there’s a statement that the distance between particles of gases is 300 times greater than their diameters so thier sizes and masses do not affect their volume.I’m confused
Correct, the volume of the particles themselves is negligible under KMT. This ends up being a reasonable assumption at relatively high temperatures and relatively low pressures.
Chemistry John Wick has helped again
Sir what if the temperature pressure is not standard and we have to find volume according to it
then i assume your prof/teacher gave you enough information to fill out the whole ideal gas law (nRT=PV)
Could Oxygen not be the unknown gas? It has an amu of 16 too
oxygen is O2, weighs 32
@@ProfessorDaveExplains its true, i forgot this! Thank you Dave
l have two gas
1 hydrogen
2 oxygen
suppose l filled equal volume of both two gases in a balloon keeping temperature and pressure at constant .... here outer pressure is 1kp .....and both have same kinetic energy
Now oxygen has more mass than hydrogen then oxygen should apply more pressure on container
if it happens then how both two has have same volume
Mr. dave please help me
pressure is not dependent on the identity of the gas, all ideal gases are treated the same regardless of what the gas is
Mr. dave l am not talking how they treated but l want to know exactly
For a few minute only forget all the law of boyle, avagadro etc.
Imagine in your mind
Two balloon one with hydrogen and second with oxygen
Particle of both have same kinetic energy and outer pressures is same so internal pressure must be same but oxygen have more mass than hydrogen so this balloon should have more pressure then how volume is same
l want to talk face to face then you understand what's my problem is
Mr. dave please do something for this problem
because they have more mass they have more inertia and therefore a lower average velocity.
@@ProfessorDaveExplains but both have same kinetic energy
yes, well average KE anyway, which depends on both mass and velocity. higher mass but lower velocity can result in the same kinetic energy.
SUPER healthy 💕
I can't find stepwise reaction
I am so confused by the Molar volume of gases calculations. Like getting from mass to moles to litres :(((
nice
But the book says 24 dm3 or 24 L im lost... :( V=molesx24
Those are equivalent.
@@ProfessorDaveExplains Thank you for yoy reply! :) Where I am lost is, in the video, you mentioned 1 mole of gas occupies 22.4 L, textbooks mention 24 L.
Hmm, no it's definitely 22.4 L at STP. Give it a google. Your book is either wrong or using different units or conditions.
Ohhhhh I've got it now!!! Sorry my misunderstanding..
STP 22.4 L and RTP 24 L. Again, thanks so much!! :)
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