Chemistry Help please ?!?

Hey Regine!....Welcome to Yahoo Answers. pi3pt141 is right and I was going to pass this by but since you said please explain I thought I'd put in my two cents. The kinetic molecular theory is really pretty simple and is easy to visualize. You've got these really tiny little guys bouncing all over the place and every time they hit the side of the container they're in (or someone who's in the container) they create a force against the thing. Since you've got billions hitting the thing at the same time, there's a force on the walls of the container, or anything that's inside the container; we call that force pressure. The more little guys you have, the more hits and the more pressure. If you shrink the size of the container (volume), you pack them into a smaller space and more of them hit the walls at the same time, (pressure goes up). If you give them more energy (heat them), they move faster and hit harder,(the pressure goes up). If you give them more volume to bounce around in, then fewer of them hit the sides of the container at any one time (volume goes up; pressure goes down).

As for Van Der Waals equation, it's an equation that fixes the lies in the kinetic theory. The kinetic theory assumes that the gas particles have no size; they're just little points of energy that go around bopping stuff and they aren't affected by the other guys. Actually of course, the molecules do have volume but ordinarily compared to the space they travel around in, they're so small that their volume can be ignored. The problem is when you pack the into a really small space they get to be really close together and their size affects the amount of space they have to move in. Finally, when they're packed that close together, they begin to feel the electrostatic attraction between them. Van der Waals equation introduces fudge factors to correct for the errors created by assuming there's no attraction between the molecules and there's no size. I hope all this helps; it really is pretty simple and if I haven't made it any clearer it's me and not the theory.

By the way, and you don't have to read this, the way Van der Waals got his constants for the various gasses is he performed experiments with the various gasses at very high pressures and very small volumes, measured the differences between what he got and what the gas equations predicted he should get. Then he put in numbers (fudge factors) to make the answers come out to be the same. It's sort of like shooting first and then drawing the circles.

question 1 . A is definately wrong as there is no above.

The answer is D . PV=nRT. so P and V are inversely proportional not directly proportional .

ie P= (nRT) x 1/V (divided both sides by V to get P and V on opposite sides of equal sign to determine their relationship)

question 2

Van der wal forces are all about attractions and repulsions between various types of molecules and bonding so the answer is D.

Nb Chemistry

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LOL he deserved an A but I am pretty sure that Hell is not freezing over......