5P-Kinetics Flashcards
What’s activation energy
The minimum amount of energy needed for particles to collide and break bonds to start a reaction
Why do most the collisions particles have not lead to a reaction
These collisions lack energy or particles have the wrong orientation
Maxwell Boltzmann distribution curve at low temp
Graph become skinny
Maxwell Boltzmann distribution curve for high temp
Curve is stretched
What’s rate of reaction
The time taken for product to be formed
How does temp change effect rate of reaction
Increases energy of molecules, more molecules have energy equal to or greater than the activation energy, more successful frequent collisions
According to Maxwell Boltzmann’s curve how can a small temp increase lead to a large increase in rate of reaction
Shaded area under curve represents number of particles, the curve shifts right as temp increases, average kinetic energy of particles increases, large number of particles have energy greater than or equal to activation energy, more frequent successful collisions
How does change in concentration effect collision frequency
More particles present in an given volume, collisions are more likely, more successful collisions, rate of reaction increases
How does change in gas pressure effect collision frequency
More particles in a given volume, collisions are more likely, more successful collisions, rate increases
What’s a catalyst
Increases the rate of a chemical reaction without being changed in chemical composition or amount
How do catalysts work
Provide and alternative reaction route of lower activation energy
Using Maxwell botzmanns distribution curve how does a catalyst increase the rate of reaction for a gas
Catalysts lower activation energy, more particles have enough energy to collide, more frequent successful collisions
