Hi. In my opinion, they cannot be spheres. Because you cannot cover the whole space using spheres and there will be unoccupied volume between them. Therefore by that assumption, the total volume will not match the volume you found the value for the volume per molecule.
Yepp, no change in content for the temperatuee, gas, and Thermodynamics chapter! Only difference are chapter and subtopic numbers (which we haven't got a chance to update yet) 😅
you are the best tr ever thx a lot
Hi. In my opinion, they cannot be spheres. Because you cannot cover the whole space using spheres and there will be unoccupied volume between them. Therefore by that assumption, the total volume will not match the volume you found the value for the volume per molecule.
we are just assuming that because we dont study the complex physics at molecular level
Thankss Miss
Thanks
how do we know that the molecules occupy space in cubic form...it can be spherical aswell....and then in that case how can we find
The cube shape is one assumption - for sphere shape, you would use the volume of a sphere:
V = 4/3πr^3, and the distance between two atoms would be 2r
Is this updated to the 2022 syllabus?
Yepp, no change in content for the temperatuee, gas, and Thermodynamics chapter! Only difference are chapter and subtopic numbers (which we haven't got a chance to update yet) 😅
@@ETphysics Not a problem at all! 😊