Monitoring and Controlling Chemical Reactions Flashcards
how do you work out the rate of a reaction?
workout how fast the products are being formed or how fast the reactants are being used up
does the rate of reaction stay the same throughout the whole reaction?
no, it starts faster and slows
why does the rate of reaction decrease over time?
as more reactants are used up, less successful collisions take place.
What is collision theory?
in order for particles to react, they have to collide with each other with sufficient energy.
What is activation energy?
the energy required for particles to collide successfully and react
What are 4 factors that effect rate of reaction?
temperature
conc/pressure
surface area
catalyst
why does increased temperature increase the rate of reaction?
the particles have more energy so they collide successfully more often
Why does increasing the concentration or pressure increase the rate of reaction?
there are more reactant particles in the same volume so the frequency of successful collisions increases
Why does increasing the surface area increase the rate of reaction?
there are more particles exposed and therefore more particles are able to react, increasing the frequency of successful collisions
What are catalysts?
substances that speed up a reaction without being used up
How do catalysts increase rate of reaction?
they create an alternate pathway with less activation energy, meaning there are more successful collisions
What are 3 examples of catalysts?
enzymes
cobalt
nickel
Transition metals make good catalysts, true or false?
true
