Making a reaction go faster-Part 1

Question 1

according to collision theory, reactant particles have to

Answer 1

collide with sufficient energy before they can react

Question 2

collisions that result in a reaction are called

Answer 2

successful collisions

Question 3

if the concentration of a solution increases, the rate increases because

Answer 3

the frequency of collisions between reacting solute particles also increases as they are closer together and there are more of them in a given volume
so the frequency of successful collisions increases so the rate of reaction also increases

Question 4

if the pressure of the gaseous mixture is increased, then

Answer 4

there will be more reactant molecules in a given volume, meaning they are closer together, so will collide more often. the frequency of successful collisions will increase, and the rate of reaction increases

Question 5

changing the pressure has…………………………..effect on reactions in the solid or liquid phase
this is because

Answer 5

virtually no effect
because the volume of solids and liquids changes very little when they are put under pressure, so their particles do not move closer together

Question 6

for heterogeneous reactions involving a solid, a large srface area will result in

Answer 6

a faster rate of reaction

Question 7

for reactions where a solid reacts with a liquid or gas, we can increase the rate by…………..
this is because…………………….

Answer 7

powdering the solid
this is because the liquid or gas reactant particles or molecules can only react with solid particles on the surface, so increasing the surface area by powdering the solid will mean more collisions occur, so the frequency of successful collisions will also increase, therefore meaning the rate of reaction increases

Question 8

solid catalysts can also be………………….to increase their effectiveness

Answer 8

be powdered to increase surface area