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PhiJ
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Does anybody know the average velocity of a particle in solution at rtp?
Phij said:The idea was ions in the body.
PhiJ said:Hmm... Another imposible problem. Should have thought about the cell membrane. That will slow things down a bit!
I thought the laws were derived from ideal gas equations assuming that particles had no attraction between them, no energy loss, small particle size etc.. If they have attraction between them, then the derivation, and hence the formulae will be wrong won't they? Then again, I may be remembering it wrong, as its a year since I was taught it.
The average velocity of a particle in solution at RTP can be calculated using the formula v = sqrt(3RT/M), where v is the average velocity, R is the gas constant, T is the temperature in Kelvin, and M is the molar mass of the particle.
As the temperature increases, the average velocity of a particle in solution at RTP also increases. This is because an increase in temperature leads to an increase in kinetic energy, causing the particles to move faster and therefore have a higher average velocity.
Yes, the size of the particle does affect its average velocity in solution at RTP. Smaller particles have a higher average velocity compared to larger particles at the same temperature, due to their smaller mass and therefore higher kinetic energy.
No, the average velocity of a particle in solution at RTP cannot be negative. Velocity is a vector quantity, meaning it has both magnitude and direction. In a solution, the average velocity of the particles will always be positive, as they are constantly moving in a random direction.
The average velocity of a particle in solution at RTP is directly proportional to its diffusion rate. This means that as the average velocity of the particles increases, their diffusion rate also increases. This is because a higher average velocity means the particles are moving faster and are more likely to collide and diffuse through the solution.