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- 1. Multiple Choice
Equilibrium is reached when the forward reaction and the reverse reaction happen at the same time.
True
False
- 2. Open Ended
The reaction produces 1.6 g of gas in 30 seconds.Calculate the mean rate of the reaction in the first 30 seconds
- 3. Multiple Choice
Complete the equation for the reaction.
CaCO3 + 2HCl ⟶ ________________________________________
CaCl + CO + H2O
CaCl2 + H2O
CaCl2 + CO2 + H2O
CaCO2 + Cl2 + H2O
- 4. Multiple Choice
Why does a higher concentration increase the rate of reaction?
it increases the amount of reactants
it lowers the activation energy
it increases the energy of reactant particles
it increases the frequency of collision
- 5. Multiple Choice
Increasing pressure causes the reacting particles
to bond together
to repel from each other
gain more kinetic energy
to move closer together
- 6. Multiple ChoiceIn an exothermic reaction, heat is ...taken ingiven out
- 7. Multiple ChoiceActivation energy is required to start a chemical reaction. What is activation energy?The energy needed for a reaction to occurThe minimum amount of energy needed for a reaction to potentially occurThe energy added by a catalystThe energy possessed by the products
- 8. Multiple Choice
Which is the reactant - and why?A, as concentration decreasesB, as concentration decreasesA, as concentration increasesB, as concentration increases - 9. Multiple ChoiceAt what time the reaction reached equilibrium?t1t2t3t4
- 10. Multiple Choice
For the reaction...
SO2 + O2 ⇄ SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
to the left
to the right
to the left and right
neither left nor right
- 11. Multiple Choice
For the reaction...
SO2 + O2 ⇄ SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
increase
decrease
remain the same
double
- 12. Multiple ChoiceLe Chatelier's Principle states that....
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................moves to increase the changemoves to counteract the changedoes not change - 13. Multiple ChoiceChanges in pressure will only affect substances that are in the __________ state.gaseousliquidsolid
- 14. Multiple Choice
For the reaction...
SO2 + O2 ⇄ SO3
If the equilibrium shifts to the left, the concentration of SO3 will ___________.
increase
decrease
stay the same
triple
- 15. Multiple Choice
Why does the rate decrease during this reaction between sodium thiosulfate and dilute hydrochloric acid?
More particles per unit volume, decreased the number of successful collisions
More particles per unit volume, decreased frequency of collisions
Fewer particles per unit volume, decreased frequency of collisions
- 16. Multiple Choice
When a low pressure is used, explain the effect on the yield of ammonia.
Increases yield of ammonia
Decreases yield of ammonia
- 17. Multiple Choice
Ammonia is removed from the reaction mixture. Explain the effect on the position of equilibrium.
moves to right hand side
moves to left hand side
- 18. Multiple Choice
Explain why the solution turns cloudy.
sulfur dioxide forms a cloud
sulfur forms a solid
yellow sulfur forms a cloudy liquid
sulfur oxide forms an insoluble solid
- 19. Open Ended
Name the product that made the mixture go cloudy.
- 20. Multiple Choice
Diagram shows the apparatus set up for an experiment to determine the rate of reaction.
Which of the following techniques is the most suitable to determine the rate of reaction?
Record the time as soon as precipitate is formed
Record the time taken to obtain the maximum temperature
Record the times as soon as the cross mark cannot be seen
Record the times taken for the change of the pH value until a fixed pH value is obtained
- 21. Multiple ChoiceWhy don't all collisions between particles cause a reaction?the particles also need to collide with a catalystnot all the particles collide with enough energynot all the particles collide at a high enough temperaturethe particles need to collide with each other twice
- 22. Multiple Choice
Which factors affect the rate of a reaction?
temperature
concentration
surface area
pressure
catalyst
- 23. Multiple Choice
Aqueous sodium thiosulfate reacts with dilute hydrochloric acid. Increasing the concentration of sodium thiosulfate increases the rate of reaction. Which statement explains this observation?
The particles are closer together and collide more frequently.
The particles are closer together and collide with more energy.
The particles have a greater surface area and collide more frequently.
The particles have more energy and collide more frequently.
- 24. Multiple ChoiceA reaction takes 90 seconds to finish.
In 30 seconds 21 cm3 of gas is made.
In 60 seconds 38 cm3 of gas is made.
In 90 seconds 50 cm3 of gas is made.
Calculate the rate of reaction between 30 and 60 seconds.0.98 cm3/s0.57 cm3/s0.63 cm3/sother answer - 25. Multiple ChoiceA reaction takes 90 seconds to finish.
In 30 seconds 21 cm3 of gas is made.
In 60 seconds 38 cm3 of gas is made.
In 90 seconds 50 cm3 of gas is made.
Identify the time period in which the rate of reaction is the fastest.Between 0 and 30 secondsBetween 30 and 60 secondsBetween 60 and 90 secondsEach time period has the same rate of reaction - 26. Multiple ChoiceIdentify the part of the graph with the fastest rate of reaction.ABCD
- 27. Multiple ChoiceIdentify the correct equation to calculate the rate of reaction.Rate of reaction = amount of products made ÷ timeRate of reaction = time ÷ amount of reactants usedRate of reaction = end time - start timeRate of reaction = amount of reactants made time ÷ time
- 28. Multiple ChoiceWhat are the two possible units for rate of reaction?g/min and min/cm3g/hour and g/cm3g/hour and min/cm3cm3/min and min/hourg/s and cm³/s
- 29. Multiple ChoiceHow could you measure the rate of a reaction from a graph?Darw a tangentCalculate the gradientDraw a tangent to the curve and calculate the gradient.Take a mean value
- 30. Multiple ChoiceWhat is the activation energy?Energy required to reactivate.Minimum amount of energy required to react.Minimum temperature required to react.Maximum energy in a collision.
- 31. Multiple ChoiceHow do catalysts speed up reactions?Provide alternative reaction route of lower activation energy.Provide alternative reaction route of higher activation energy.Provide reaction route of higher temperature.Provide alternative reaction route of higher transparency.
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