reaction won’t take place between two particles unless they collide in the right direction with enough energy
1 of 18
what's activation energy?
minimum amount of energy particles need to react. Particles need this to break the bonds to start the reaction.
2 of 18
what's the enthalpy change?
difference between the enthalpy of the reactants and the enthalpy of the products
3 of 18
what makes a reaction exothermic?
If the products have a lower enthalpy than the reactants
4 of 18
what makes a reaction endothermic?
If the products have a higher enthalpy than the reactants
5 of 18
using collision theory, state what happens if you increase the temperature of a reaction
molecules have more kinetic energy and will move faster. More molecules have at least the activation energy and can react. Maxwell-boltzmann curve moves to the right
6 of 18
using collision theory, state what happens if you increase the concentration of the solution
particles in solution will be closer together and can collide more often. More collisions equals more chances to react
7 of 18
using collision thwory, state what happens if you increase the pressure of a reaction involving gases
more molecules in total to collide in a given volume. More molecules with energies above activation energy
8 of 18
state 2 features of dynamic equilibrium
rate of forward reaction is same as rate of backwards reaction. Concentrations of reactions and products remain the same
9 of 18
what does le chatelliers principle state?
when reaction conditions are changed at equilibrium, the position of equilibrium will shift to counteract this change
10 of 18
what happens to the position of equilibrium when we change the concentration?
increasing conc of a reactant makes more product. Increasing conc of a product makes reverse reaction go faster
11 of 18
what happens to the position of equilibrium when we change the pressure?
increasing pressure shifts equilibrium to side with fewer gas molecules. Decreasing pressure shifts equilibrium to side with more gas molecules
12 of 18
what happens to the position of equilibrium when we change the temperature?
increasing temperature, equilibrium shifts in endothermic (+ive ∆H) direction. Decreasing temperature, equilibrium shifts in exothermic (-ive ∆H) direction.
13 of 18
what's the equation for ethanol production?
C2H4(g) +H2O↔C2H5OH ∆H=-46kJmol
14 of 18
what are the conditions for ethanol production?
pressure of 60-70atm, temp of 300o.Phosphoric acid catalyst
15 of 18
how do you get a 95% overall yield if only 5% is converted each time?
gases pass through the catalyst. Unreacted ethene is separated from the liquid ethanol and recycled back into the reactor
16 of 18
what's the equation for methanol production?
2H2(g)+CO(g)↔CH3OH ∆H=-90kJmol
17 of 18
what are the conditions for methanol production?
pressure of 50-100atm, temp of 250o. catalyst mix of Cu, ZnO and aluminium oxide
18 of 18
Other cards in this set
Card 2
Front
what's activation energy?
Back
minimum amount of energy particles need to react. Particles need this to break the bonds to start the reaction.
Comments
No comments have yet been made