Skip to Content
Introducing new Paper mode
No student devices needed. Know more
20 questions
Show Answers
See Preview
- 1. Multiple-choice1 minute1 ptWhat is the rate of a chemical reaction? Choose 2.How quickly the reactants in a reaction are used upHow quickly the reactants in a reaction are madeHow quickly the products in a reaction are usedHow quickly the products in a reaction are formed
- 2. Multiple-choice1 minute1 ptHow do we calculate mean rate of reaction?quantity of product made/time takentime taken/quantity of product made
- 3. Multiple-choice1 minute1 ptWhat are the two possible units for rate of reaction? Choose 2
s/g
g/m
cm³/s
g/s
m/s - 4. Multiple-choice1 minute1 ptOn a rates graph, what type of line shows the reaction has ended?SlopedCurvedStraightVerticalHorizontal
- 5. Multiple-choice1 minute1 ptWhat is "collision theory"?Reactions only occur when particles collide with sufficient energyCollisions occur when particles collide with no energyCollisions mean that particles hit each other gently
- 6. Multiple-choice1 minute1 ptWhat factors can affect the rate of a reaction? Choose 4TemperatureSurface area of a solidConcentration in solution, pressure of gasesBigger beakerPressure of gases
- 7. Multiple-choice1 minute1 ptState the effect of increasing the surface area on the rate of a reactionIncreasesDecreasesStays the same
- 8. Multiple-choice2 minutes1 ptWhy does increasing surface area increase the rate of a reaction?Less particles available to collide, so more frequent effective collisions.More particles available to collide, so more frequent effective collisions.Less particles available to collide, so less frequent effective collisions.More particles available to collide, so less frequent effective collisions.
- 9. Multiple-choice1 minute1 ptIncreasing the concentration …........................ the rate of reactionIncreasesDecreasesStays the same
- 10. Multiple-choice1 minute1 ptWhy does increasing concentration increase the rate of reaction?More particles in more space, so more frequent effective collisions.More particles in same space, so less frequent effective collisions.More particles in same space, so more frequent effective collisions.
- 11. Multiple-choice1 minute1 ptHow does increasing gas pressure change the rate of reaction?IncreasesDecreasesStays the same
- 12. Multiple-choice1 minute1 ptWhy does increasing gas pressure increase the rate of a reaction?Less space for the particles to move, therefore more frequent collisionsMore space for particles to move, so more collisions
- 13. Multiple-choice1 minute1 ptIncreasing the temperature …....................... the rate of reactionIncreasesDecreasesStays the same
- 14. Multiple-choice1 minute1 ptWhat is the activation energy?The minimum energy a particle needs to reactThe maxmum energy a particle needs to react
- 15. Multiple-choice2 minutes1 ptWhy does increasing temperature increase the rate of reaction?Increases the speed at which particles move therefore more frequent effective collisionsIncreases the number of particles which have the activation energy therefore more collisions result in a reaction.Decreases the speed at which particles move therefore more frequent effective collisionsDecreases the number of particles which have the activation energy therefore more collisions result in a reaction.
- 16. Multiple-choice1 minute1 ptWhat is a catalyst? Choose 2Something which decreases the rate of a reactionIt is used upSomething which increases the rate of a reactionIt is not used up
- 17. Multiple-choice1 minute1 ptHow do catalysts speed up reactions?They provide another route for the reactionThey give particles more energy
They increase surface area
They lower activation energy - 18. Multiple-choice1 minute1 pt
Look at the graph. At what time does the reaction finish?
4 minutes
5 minutes
6 minutes
7 minutes
- 19. Multiple-choice1 minute1 pt
What would the rate be if 10g of product are produced in 20 seconds?
5 g/s
0.5 g/s
1.5 g/s
2 g/s
- 20. Multiple-choice1 minute1 pt
Increasing the pressure of a reaction in which reactants are gaseous will lead to the rate of reaction...
... decreasing
... increasing
