# Rates summary

- Created by: h98
- Created on: 24-11-15 18:02

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- RATES
- change in concentration per unit time (mol1dm-3)
- factors affecting rate
- surface area: larger surface area, more frequent and more successful collisions.
- catalyst: speeds up rate of reaction without being used up, lowers Ea by providing and altering the pathway
- temperature: higher temperature, more kinetic energy, more frequent and more successful collisions.
- concentration: higher concentration, more frequent collisions, more successful collisions.
- pressure: increase pressure, more particles per unit volume, more frequent and more successful collisions

- order of reaction
- first order: the rate of reaction is directly proportional to the concentration
- second order: the rate of reaction is proportional to the square of the change in concentration
- zero order: the rate of reaction is not affected by the change in concentration.

- rate equations
- rate = k [X][Y]2
- [X] first order [Y]2second orderdo not include zero order int this equation
- overall order: add the powers

- concentration-time graphs
- 1. label axis2.half life tells if its 1st order or not3.show minimum of 2 half lives4state the values of the half lives and the units
- calculation rate:1. draw tangent following curve 2.dy/dx include units 3.initial rate=0 seconds4.must cross line at time=0 seconds5.label axis, include units

- factors affecting rate
- surface area: larger surface area, more frequent and more successful collisions.
- catalyst: speeds up rate of reaction without being used up, lowers Ea by providing and altering the pathway
- temperature: higher temperature, more kinetic energy, more frequent and more successful collisions.
- concentration: higher concentration, more frequent collisions, more successful collisions.
- pressure: increase pressure, more particles per unit volume, more frequent and more successful collisions

- molar ratios:A+2B --> C+Dwhat is the rate of formation of the compound C if the rate of B is 10moldm-3?2:1 molar ratio, 10/2=5 moldm-3
- RATES
- change in concentration per unit time (mol1dm-3)
- order of reaction
- first order: the rate of reaction is directly proportional to the concentration
- second order: the rate of reaction is proportional to the square of the change in concentration
- zero order: the rate of reaction is not affected by the change in concentration.

- rate equations
- rate = k [X][Y]2
- [X] first order [Y]2second orderdo not include zero order int this equation
- overall order: add the powers

- concentration-time graphs
- 1. label axis2.half life tells if its 1st order or not3.show minimum of 2 half lives4state the values of the half lives and the units
- calculation rate:1. draw tangent following curve 2.dy/dx include units 3.initial rate=0 seconds4.must cross line at time=0 seconds5.label axis, include units

- RATES

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