Rate Of Reaction Flashcards
Define rate of r reaction
How fast product is formed or how fast reactant are used up
Things that can calculate/ quantify rate of reaction
1, mass loss of reactant
2, mass gained by products
3, volume of gas
4, pressure of gas
5, colour intensity
6, solution concentration
Define activation energy
1, min amount of energy to break bond so that reaction can occur
2,min amount energy colliding reactant must posses in order to get reaction
What are the collosin theory requirements
1, collide with sufficient energy to break bond between reactant
2, Collide with correct orientation to break bond between reactant
Rate Of Reaction can be increased by ?
Increase :
Surface area of reactant
Pressure of gaseous product
Tempreture of reaction system
Catalyst
Increasing surface area of reactant
1 greater reactant collision
2 increase in frequency of collusion
3 increase number of successful collusion
Increasing surface area of reactant
1 greater reactant collision
2 increase in frequency of collusion
3 increase number of successful collusion
Increasing the concentration of reactant
1 increase in solute particles per unit volume
2 frequency of collusion
3 number of successful collusion in a given time
Increase in pressure of gaseous reactant results in ?
1 increase number of gas particles per given volume
2 increase frequency of collusion
3 increase successful collusion in a given time
Increasing temperature of the reaction increase the:
1 Frequency of collusion
2 PROPORTION of successful collusion
3number of collusion in given time
Adding catalysts does what ?
1Provides an alternative path way with a lower activation energy
2Increase the PROPORTION of successful collusion
3 increase the number of collusion in given time
Describe closed system
Energy is exchanged with the surrounding but matter is not
Describe open system
Both matter and energy are exchanged between system and surroundings
Describe open system
Both matter and energy are exchanged between system and surroundings
Describe reversible reaction
Reaction where products can be converted back to the reactant
Describe irriversable reaction
Reaction where products can’t convert to reactant
When is a reaction most likely to be reversible
If the activation energy for the forward and reverse are similar
When is a reaction most likely to be reversible
If the activation energy for the forward and reverse are similar
Describe when equlibrium has been achieved in a reaction
When the rate of reaction for forward and reverse are equal
When can equlibrium be achieved
Only on closed system
Define the state of dynamic equlibrium
The rate of forward reaction equals to the reverse reaction
How do we work out equlibrium constant
Concentration of products decided by concentration of reactant both with cofficents
Constant equlibrium sign
K č
What affects the equlibrium constant and how?
Temperature
Temp increase Kč decreases
Temp decrease Kč increases
