Rate Of Reaction Flashcards
What is the rate of reaction?
How quickly the reactants turn into the products
How do you calculate the rate of reaction?
Quantity or reactant used or product formed/ time taken
How do you calculate the volume of gas produced?
The reaction of the mixture is connected to a gas syringe or measuring cylinder (upside down)
What is volume measured in?
cm^3
How do we calculate the mean rate at a specific point on a graph?
Draw a tangent and calculate the gradient
What is the unit of rate of reaction?
g/s
What does a steep gradient mean in rates of reaction?
The reaction is happening quickly
What is collision theory?
For a reaction to occur, the particles need to collide. When the particles collide, they need to have enough energy to react. This is known as the activation energy.
How can you increase the rate of reaction?
Increasing the frequency of collisions
Increasing the energy of particles when they collide
What factors increase the rate of reaction?
Temperature, concentration of solutions, pressure, surface area
How does increasing the temperature increase the rate of reaction?
Particles move faster, leading to more frequent collisions. Particles have more energy so more collisions result in a reaction.
How does increasing the concentration of solutions increase the rate of reaction?
There are more reactant particles in the reaction mixture so more frequent collisions.
How does increasing the pressure of gases increase the rate of reaction?
Less space between particles means more frequent collisions.
How does increasing the surface area of solids increase the rate of reaction?
Only surface particles are able to react so the greater the surface area, the more reactant particles are exposed and the more frequent the collisions.
What are catalysts?
Catalysts speed up the rate of reaction without being used up in the process, they provide a different reaction pathway that has a lower activation energy. More particles will therefore collide with enough energy to react so more collisions result in a reaction.
