| The equilibrium law | kc = products 2 / reactants2 |
| How to calculate rate? | change in conc/time |
| The definition for activation energy | The minimum energy req to for reactant to react |
| The effect of conc on reaction rate | increased conc gives more molecules in the same volume , more chance of collisions so more successful collisions per unit time |
| The effect of pressure on rate of reaction | The same no of molecules occupy a smaller volume so more successful collisions per unit time |
| Define Catalyst | A catalyst lowers the activation energy of the reaction by providing an alternate route |
| Homogenous catalyst | Same physical state of all reactants |
| Heterogenous catalyst | Different physical state from the reactants |
| Uses of catalysts | - reducing energy consumption
-cost efficient
-biological catalysts
-industry |
| Key things to remember in the boltzman curve | - axis names energy and number of molecules
- the higher temp shift to right a greateer proportion of molecules exceed activation energy so more collision so a faster r of r
- write the crocoadile |
| Dynamic equilibrium | 1. the concentration of the reactants and products remain the same
2. the rate of the forward reaction is the same as reverse
3. closed system |
| L e Chatelier's principle | the position of the equilibrium will shift to minamise the change |
| The effect of conc on equilibrium | increasing conc of reactant will shift right
decreasing conc of products will shift left |
| Increasing H+/ adding an acid | You would add an alkali * mention colour changes * |
| The effect of pressure on equilibrium | increase shifts to fewer
decrease shifts to greater |
| The effect of temperature on equilibrium | - look at the sign as that is the forward reaction
-increase temps shifts in endo
-decrease temp shifts in exo as - |
| The equilibrium law | kc = products 2 / reactants2 |
