The pressure on a sample of hydrogen is doubled, while its temperature is kept unchanged. What happens . . .?

Question

to the average speed of the hydrogen molecules?

Answer 1

This kind of depends on the other conditions of your experiment. By Boyle's law, PV=nRT, or pressure times volume = number of moles of gas times a constant times temperature. Since your pressure goes up, the only way to keep temperature constant is to reduce the volume of your container by half. Is that the condition of the experiment? Your gas is in a piston chamber of some sort? Generally, compressing a gas increases its temperature, so I suppose if you did this, you could measure the temperature beforehand, compress the gas and then wait until the gas cooled back down to the same temperature.

In any event, since temperature is simply the measure of the average kinetic energy of all the particles in a system, since kinetic energy itself is calclulated by knowing velocity and mass and the mass hasn't changed, at the same temperature, the gas molecules have the same average kinetic energy and therefore the same velocity, and since you don't specifically care WHICH direction they're travelling in, they are at the same speed.

Answer 2

You can keep temperature the same, by isothermal devices. Which is usually a fancy name for a room temp water bath, but p.chemists like fancy names-and I've seen ones a little more complicated. So I guess they're allowed. But since temperature is the measure of speed of molecules, nothing will happen to the average speed of the hydrogen molecules. It'll stay the same. By definition.

Answer 3

utilising the proper gasoline regulation and fixing for 10 atm of rigidity and 273 kelvin then for 5 atm of rigidity and 546 (double) kelvin, the quantity more effective through 4 cases. the most recommendations-blowing answer is D. in accordance to Charle's regulation, at consistent rigidity, quantity is instantly proportional with temperature. If temperature doubles so does quantity. If temperature drops through 1 million/2 quantity is decreased through 1/2. the most recommendations-blowing answer is A.

Answer 4

It's true! I agree with PV=nRT and TheHza (about temperature being a measure of the kinetic energy of the hydrogen).

PV=nRT can be thought of an energy balance. Since it is assumed n (amount of substance) and R (gas constant) are not changing, and the temperature doesn't change, then the right side of the equation remains constant. Therefore, the energy remains constant. Since you have the same amount of hydrogen, with the same amount of energy, it is the same speed.

Answer 5

Obviously, the gas will increase it's temperature when you increase it's pressure. But if you give it enough time, It will dissipate the heat until it equalized again to it's surrounding medium.

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