C6 Flashcards
what is gas pressure?
(prior knowledge)
the force exerted when gas particles collide with the surface of their container
what must happen before the reaction will start?
the particles must collide with enough activation energy
what does rate a measurement always have to include?
a measurement of mass or volume (of a substance) and a measurement of time
what is the definition of rate of reaction?
when the mass or volume of reactants change into products over a period of time
what is the definition of concentration?
the mass of solute within a certain volume (of solvent)
why is activation energy required?
to break bonds in the reactants
when is a reaction fastest?
at the start
why does a reaction slow down as it progresses?
there are little reactants left –> so there are less frequent successful collisions
dk the question to this answer
high concentration of reactant particles so more successful frequent collisions
what happens to the rate of reaction when the concentration is increased? why?
also increase because there are more reactant particles per unit volume
what happens to the mass or volume of a product if the concentration is increased?
stays the same
define random error.
variability between different measurements
what happens to the rate of reaction when you increase concentration? why?
increases - because there are more reactant particles in the same volume –> so there are more successful frequent collisions –> so the rate increases
when does a reaction stop?
when 1 or more reactants has been used up (limiting reactant)
what graph do we use to present continuous data?
line graph
state 2 ways to increase the rate of reaction?
- increase the temperature
- increase concentration of reactants
why is carbon dioxide a gas at room temperature?
because it is a simple covalent molecule with weak intermolecular forces between the molecules so little energy is needed to break the forces
define intervals
quantity between readings
what are the 5 factors that affect rate of reaction?
- concentration
- temperature
- surface area
- pressure
- catalyst
how does concentration affect the rate of reaction?
there are more reactant particles in a given volume so there are more successful frequent collisions
how does temperature affect the rate of reaction?
there is more kinetic energy in the reactant particles so they move faster, therefore there are more successful frequent collisions
how does surface area affect the rate of reaction?
there are more surfaces for the reactant to collide with so there will be more successful frequent collisions
how does pressure affect the rate of reaction?
there is a greater chance of collisions with high pressure as reactant particles have a smaller space, therefore there will be more successful frequent collisions
how does a catalyst affect the rate of reaction?
lowers the activation energy by finding an alternative pathway
what is a closed system?
when no products can leave and no new reactants can enter
what is meant by ‘yield’ in a reaction?
how much product you actually make in a reaction
what is a dynamic equilibrium?
when the forward and backward reaction happens at the same rate
what happens to concentration in a dynamic equilibrium?
stays constant
what kind of system does a dynamic equilibrium ONLY happen in?
ONLY happens in a closed system
What does Le Chatehier’s principle state?
Increasing temperature favours the endothermic reaction and Decreasing temperature favours the exothermic reaction
What side does pressure favour?
The side with the fewest moles.
Which catalyst is used when ammonia is produced from nitrogen and hydrogen.
Iron
