REACTION RATES

Question 1

RATE of REACTION - definition

Answer 1

How fast the reactants are changed into products , measures CHANGE in CONCENTRATION of PRODUCTS per unit TIME

Question 2

RATE of REACTION - found by measuring how QUICKLY

Answer 2

• amount of REACTANT USED UP
• amount of PRODUCT FORMED

Over given time !!!

Question 3

5 FACTORS that effect RATE

Answer 3

1) Temperature

2) Catalyst

3) Pressure

4) Surface Area

5) Concentration

Question 4

EFFECTIVE SUCCESSFUL COLLISION

Answer 4

Reacting particles COLLIDE with SUFFICIENT ENERGY , at a certain SPEED

Question 5

ACTIVATION ENERGY

Answer 5

MINIMUM amount of ENERGY particles need to REACT

Question 6

CATALYST -

Answer 6

Increase rate of reaction without being used upon- has same mass throughout

! Provides ALTERNATIVE REACTION PATHWAY of LOWER ACTIVATION ENERGY

So collision needs LESS ENERGY to be SUCCESSFUL

More PARTICLES have energy >= ACTIVATION ENERGY - more EFFECTIVE SUCCESSFUL COLLISIONS

Question 7

Surface Area

Answer 7

SURFACE AREA Inversely proportional to PARTICLE SIZE - smaller particles = faster reaction

! Larger CONTACT AREA - MORE PARTICLES of the solid are AVAILABLE for COLLISIONS

! FREQUENCY INCREASES - more ES COLLISIONS

Question 8

Concentration

Answer 8

MORE particles in FIXED VOLUME - CLOSER

! RATE of COLLISIONS INC

Question 9

TEMP

Answer 9

Particles have more energy - move FASTER - more frequent collisions too

MORE ENERY THAN ACTIVATION ENERGY

Question 10

PRESSURE - gases

Answer 10

CLOSER TGT