Reactivity Flashcards
What 4 factors speed up the rate of reaction?
1) Increasing temperature
2) Increasing surface area (splitting up the products)
3) Increasing the pressure
4) Increasing the concentration
Activation energy is…
The minimum amount of energy required for particles to start reacting
How does temperature affect the rate of reaction?
Increasing the temperature gives Thermal Energy to particles, which then becomes Kinetic Energy. The particles then Move Around More, creating More Collisions Between Particles, Speeding up the Rate Of Reaction
How does increasing the pressure affect the rate of reaction?
Increasing the Pressure leaves Less Volume for Particles to Move in, meaning More Collisions occur as there is nowhere else to go, consequently Speeding up the Rate Of Reaction
Changing the concentration does not affect the rate of reaction. True or False?
False - Increasing the Concentration of a product Increases the Amount Of Particles present. That makes it Easier for Collisions to occur, thus Speeding Up the Rate Of Reaction
If I have large chunk of magnesium and I split it into 4, how will it affect the rate of reaction with oxygen?
Splitting the magnesium up gives multiple extra sides, as the surface area is increased. This gives more space for the oxygen to react with the magnesium, so the rate of reaction speeds up
An exothermic reaction is when heat leaves the chemical reaction. True or False?
True - it expels the extra energy it has, so it is released as thermal energy
An endothermic reaction is when heat leaves the chemical reaction. True or False?
False - it takes in energy from its surroundings to reach its activation energy, causing the air around it to turn cold
What is the symbol for a reversible reaction?
\ (but I’m gonna write --\ for ease)
GIve the compound? that is used a lot in reversible reaction examples
Ammonia - NH3
The haber thing means what?
Reversible reaction
What is Le Chatelier’s principle?
That whatever change you enact in a closed environment on a reversible reaction, the reaction will do the opposite.
N2 + H2O --\ NH3
The left side is endothermic. The right side is exothermic.
If I increase the temperature on the equilibruim, which side will it turn to?
The left side. Because it wants to become colder like the fusspot it is, so increasing heat will make lots of nitrogen + water (also, as it is hot, it is quick)
What is a dynamic equilibrium
GO CHECK
N2 + H20 --\ NH3
If I increase the pressure a lot, what will happen?
1) count the molecules!
2 molecules --\ 1 molecule
In the decreasing space, the fusspot reaction wants less space, so will form more ammonia as 1 molecule takes up less space.
