topic 6 Flashcards
for a chemical reaction to occur particles must : (2)
- collide in the correct orientation
- with enough energy for a reaction to take place called the activation energy
what is the rate of reaction
the speed at which the reaction takes place
ways to speed up chemical reactions
- lower volume (increase pressure)
- increase number of particles
- increasing temperature
- increasing surface area
- using a catalyst
what does increasing concentration mean, and how is it achieved
increases number of solute particles per unit volume, achieved by adding more particles
what does increasing the concentration do in terms of particles
increases the frequency of collisions and rate of reaction
what does increasing pressure mean, and how is it achieved
increases the number of gas particles per unit volume. achieved by adding particles or reducing container volume
what does increasing pressure do in terms of particles
increases the frequency of collision and rate of reaction
what does increasing temperature do do particles
increases the kinetic energy allowing more particles to collide more frequently and with enough energy to overcome the activation energy,
what does increasing surface area mean
means more particles are exposed on the outside, fewer unexposed particles in the middle.
what are catalysts and what do they do to rate of reaction in chemistry
are chemicals that speed up the rate of reaction without being used up or changing at the end of the reactions. they do this by allowing the reactant particles to collide more easily making the collisions more successful
what happens to the rate of reaction as reactions take place
rate of reaction decreases because as more products are formed, concentration of reactants decrease.
what happens to bonds when making new particles
bonds between reactant particles must be broken
about an endothermic reaction
- energy, bonds, temp
- absorbing energy
- breaking bonds = absorbing energy
- temperature of surrounding decreases
about an exothermic reaction
- energy, bonds, temp
- involves releasing energy
- making bonds = releasing energy
- temperature of surroundings increase
what does it mean in terms of bonds when a overall reaction is exothermic
energy absorbed to break bonds < energy released to make bonds
what does it mean in terms of bonds when a overall reaction is
endothermic
energy absorbed to break bonds > energy released to make bonds
what is enthalpy , and units
the change in energy between reactants and products
kj/mol or kj mol -1
enthalpy equation
total energy of bonds broken - total energy of bonds made
