equilibria, rate of reaction
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what is exothermic reaction
release thermal energy, surrounding heat up
what is endothermic reaction
take in energy, surroundings cool down
enthalpy change in endo and exo reactions
in exo its negative, endo is positive
what is the transfer of thermal energy during a reaction called?
enthalpy change
what is activation energy
the minimum energy that colliding particles must ave to react
endo and exo in terms of bonds
endo is in bond breaking, in which energy is used to do so and exo is in bond making, no energy is needed to make bonds
what is the law pf energy to break or make bonds
always same amount of energy needed to produce or make bonds
what does this symbol represent? ⇌
reversible reaction, occurs in both the forward and backward direction
what happens if forward reaction is exo
backward is endo
what colour change occurs if anhydrous copper sulfate was added to water
white to blue
what colour change occurs in anhydrous cobalt chloride was added to water
blue to pink
what is dynamic equilibrium
Revirsable reactions that take place in a closed system -the forward and backward reactions occur at same rate -the concentrations of reactants and products are no longer changing
what is the process to reach dynamic equilibrium
at start there are reactants only no products, rate of reactants being used up increases and rate of products being used up decreases rate of forward and backward reaction is the same
what happens to rate of reaction if temperature increases
The rate of reaction is faster/ increases because kinetic energy is given to molecules therefore increasing the number of collisions per second the particles gain more energy and move faster. This means that they collide more often. If the temperature is decreased, the particles have less energy, move more slowly and collide less often
what happens to the position of equilibrium when temperature increases
shifts to the endothermic side
what happens to the position of equilibrium when temperature decreases
shifts to the exothermic side
what happens to the position of equilibrium when we increase concentration
position shifts to the opposite side in which the concentration was increased to balance the equation again
what happens to rate of reaction if we increase pressure
increases rate of reaction because there are more molecules per centimeter cubed therefore there are more collisions per second, the number of particles in a given volume also increases an so the rate of reaction increases.
what happens to the position of equilibrium once we increase pressure
shift to the side with less molecules
what happens to the position of equilibirum if a catalyst is added
forawrd and backward reaction are sped up however there is no effect on position
what is the symbol equation for the production of ammonia in the haber process
N2(g) +3H2(g) <–>2NH3(g)
what are the sources of hydrogen and nitrogen in the Haber process
hydrogen- methane nitrogen- air
what are the typical conditions in the Haber process
450 celsius 20000kPa/200 atm iron catalyst
what is the symbol equation for the conversion of sulfur dioxide into sulfur trioxide in contact process
2SO2(g) + O2(g) <—> 2SO3(g)