https://padlet.com/hew_zi_heng/e1jeu3jlzkol Made with a quick smile en-us 2017-03-30 04:08:02 UTC 2017-03-30 04:42:22 UTC hello@padlet.com hew_zi_heng https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596414 1. Temperature
2. Pressure
3. Concentration
4. Surface area
5. Prescence of a Catalyst]]> 2017-03-30 04:09:02 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596414 hew_zi_heng https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596427 Collisions of particles affect the Speed of Reaction]]> 2017-03-30 04:09:14 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596427 hew_zi_heng https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596643 1. Change in temperature
2. Formation of precipitate
3. Colour change
4. Change in the pH
5. Pressure/Volume of gas collected
6. Mass of Reaction Mixture]]> 2017-03-30 04:12:36 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596643 joshua_yew_jek_yong https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596673 Increase of temperature will increase the rate of reaction

The increase in temperature will mean that the particles have more kinetic energy .
- This increases the frequency of effective collisions between particles 
- This also increases the energy of effective collisions between the particles, so that more particles exceed the reaction's activation energy

Thus increasing the frequency of effective collisions increases the rate of the reaction]]> 2017-03-30 04:12:59 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596673 afiq_prasanto https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596717 ↑ in pressure of guess,
↑ in rate of reaction.

↑ in pressure of gas will force particles closer together,
↑ frequency of collisions

∴ 
↑ in frequency of effective collisions,
↑ in rate of reation.]]> 2017-03-30 04:13:35 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596717 afiq_prasanto https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596800 ↑ in surface area of solid,
↑ in rate of reaction.

↑ in surface area of a solid reagent,
↑ in area over which collisions between two reacting chemicals take place,
↑ frequency of collisions.

∴ 
↑ in frequency of effective collisions,
↑ in rate of reaction.]]> 2017-03-30 04:15:17 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596800 hew_zi_heng https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596897 Increase in concentration = particles are closer together. There are mrore particles per unit volume.

This means the particles will collide more frequently and effectively]]> 2017-03-30 04:16:52 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163596897 hew_zi_heng https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163597008 1. Reduces the activation energy needed by allowing the reaction to take place via an alternative pathway
2. Lowering Ea = Less effective collisions needed]]> 2017-03-30 04:18:43 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163597008 hew_zi_heng https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163597100 Particles collide together for reactions to take place. When they collide, the particles break up and form new compounds for the reaction]]> 2017-03-30 04:20:27 UTC https://padlet.com/hew_zi_heng/e1jeu3jlzkol/wish/163597100