9A.3 Flashcards
describe a Maxwell-Boltzmann distribution graph
- the curve is never symmetrical
2. it starts at the origin and finishes near the x-axis asymptote
compare a Maxwell-Boltzmann distribution graph of two different temperature
- both graphs have the same area under the graph
2. and the higher temperature peak would be lower and more to the right
how do you label the x-axis and the y-axis in a Maxwell-Boltzmann distribution graph
y-axis = fraction o molecule with energy x-axis = energy
how do we find the number of molecules that have enough energy to successfully collide
by looking at the area under the graph from the activation energy mark
how does the temperature affect the rate of reaction and why
the rate of collisions increases, because an increase in temperature increases the fraction of molecules that possess the required activation energy therefore more successful collisions per second
is the fraction of collisions with energy equal or greater than Ea and the fraction of molecules with the same energy =
that is not true but with very high energies and a small fraction the difference isn’t as much
in the gas phase, a single molecule might have how many collisions per second
10^9 or 10^10 depending on the size
what are the two stages for the reaction in a solution
- molecules have to come together by a process of diffusion, in the same solvent cage
- they have to react
what is a solvent cage
it happens in low-to-mid concentrations where the solvents are more dominant than the solute so they would entirely cover them in a solvent cage
are collisions in solution faster than the collision in the gas phase
gas-phase usually has more collisions, but if the solute molecules get trapped in a solvent cage they can react together and collide similarly to the collisions in the gas phase
the chances of two species meeting each other in a solution is proportional
to their concentration just as in the gas phase