chemistry topic 6

?
  • Created by: El17P
  • Created on: 22-03-23 18:07
1.what is the rate of a chemical reaction?
2. what are examples of the slowest?
3.what are examples of moderate reactions?
4. what are examples of fast reactions?
5. what does the steepness of a line on a graph tell you about the reaction?
6. what does it
1.how fast the reactants are changed into products
2.rusting or iron and chemical weathering
3. magnesium and acid
4.explosions and burning
5.the steeper the line, the faster the rate of reaction
6. the reaction is finished
1 of 9
1.what is collision theory?
2. what is activation energy?
3. what does the rate of reaction depend on?
4.how does increasing the temperature increase the rate?
1. the rate of reaction depends on collision frequency and energy transferred.
2. the minimum amount of energy particles need to break the bonds and react.
3. temperature, concentration of a solution or pressure of the gas, surface area, presence of a cat
2 of 9
5. how does increasing the concentration or pressure increase the rate?
6.how does increasing the surface area increase the rate?
7.how does using a catalyst increase the rate?
5.it will be more concentrated and so there will be more frequent collisions.
6.the surrounding particles will have more space to work on so collisions will be more frequent.
7.they decrease the activation energy by providing an alternative reaction pathw
3 of 9
1. what are the three ways to measure the rate of reaction?
2.how do you find the mean rate of reaction?
1. precipitation and colour change (observe a cross beneath), change in mass (the quicker the mass drops, the faster the reaction), the volume of gas released (measure using a gas syringe).
2.amount of reactant used or amount of product formed/time
4 of 9
rates of reaction: Magnesium and HCI to produce H2 gas
1. add a set volume of dilute hydrochloric acid to a conical flask and place on a mass balance
2.add magnesium ribbon and plug the flask with cotton wool
3.start stopwatch and record mass at regular i
4. put into a table and find mass lost for each reading.
5. plot graph and repeat with varied concentrated acid solutions. keep magnesium ribbon and acid vol controlled.
6. the graphs should show the higher the conc, the faster the reaction
5 of 9
rates of reaction: sodium thiosulfate and HCL produce a cloudy precipitate.
1.add a set volume of dilute sodium thiosulfate to a conical flask and place on a black cross.
2. add some dilute HCL to the flask and start the stopwatch.
3.time how long it takes for it to disappear
4.repeat with any one of the solutions of either reactant at different concentrations but keep the depth the same.
5. you can find the mean rate reaction from a graph by using change in y / change in x
6 of 9
1. how are some reactions reversible?
2. what happens after a while of this in a closed system?
3.what happens to the concentration if it lies to the right?
1. as the reactants react, there concs fall so the forward reaction slows, as more products are made up and their conc rise the backward reaction will speed up.
2. the forward reaction will be at an equal rate as the backward (at equilibrium)
3.conc of pr
7 of 9
1.what conditions does the position of equilibrium depend on?
2.in reversible reactions is the reaction is endothermic in one direction, what will the other direction be?
3. what is la chatelier's principle
1. the temperature, the pressure and the concentration.
2. exothermic
3. the idea that if you change the conditions of a reversible reaction at equilibrium, the system will try and counteract that change.
8 of 9
4.for example, what happens when you change the temperature?
5. what about the pressure?
6. concentration?
4. if you decrease it, the reaction will move in the exothermic direction to produce more heat, creating less products for the endothermic reaction etc
5. if increased, it moves in the direction where there's less molecules of gas, if decreased, it moves
9 of 9

Other cards in this set

Card 2

Front

1.what is collision theory?
2. what is activation energy?
3. what does the rate of reaction depend on?
4.how does increasing the temperature increase the rate?

Back

1. the rate of reaction depends on collision frequency and energy transferred.
2. the minimum amount of energy particles need to break the bonds and react.
3. temperature, concentration of a solution or pressure of the gas, surface area, presence of a cat

Card 3

Front

5. how does increasing the concentration or pressure increase the rate?
6.how does increasing the surface area increase the rate?
7.how does using a catalyst increase the rate?

Back

Preview of the front of card 3

Card 4

Front

1. what are the three ways to measure the rate of reaction?
2.how do you find the mean rate of reaction?

Back

Preview of the front of card 4

Card 5

Front

rates of reaction: Magnesium and HCI to produce H2 gas
1. add a set volume of dilute hydrochloric acid to a conical flask and place on a mass balance
2.add magnesium ribbon and plug the flask with cotton wool
3.start stopwatch and record mass at regular i

Back

Preview of the front of card 5
View more cards

Comments

No comments have yet been made

Similar Chemistry resources:

See all Chemistry resources »See all topic 6 resources »