Lesson Worksheet: Reaction Rate Measurements Chemistry • 10th Grade
In this worksheet, we will practice performing different experiments whose results can be analyzed to calculate the rate of reaction.
Q1:
Which of the following is not a viable unit for a reaction rate?
- Akg/s
- Bt/d
- CM/min
- Dh/s
- Eg/s
Q2:
The rate of a reaction can be determined by measuring changes in the physical properties of the reaction mixture. Which of the following parameters is not typically monitored to obtain a measure of reaction rate?
- ATemperature
- BVolume
- CColor
- DCloudiness
- EMass
Q3:
What is the formula for calculating the rate of a reaction from the reaction time and the amount of product formed?
- A
- B
- C
- D
- E
Q4:
Shown in the diagram is the experimental apparatus used to identify the end-point of a reaction from changes in turbidity. The average reaction rate is determined by measuring the time taken for the cross to be obscured by the product suspension.
When monitoring changes in turbidity, the cross must be viewed from directly above. How does this approach help to ensure that the experiment is repeatable?
- AThe cross is not viewed through glass, which would reduce its visibility by refracting light.
- BThe cross is not viewed through glass, which would reduce its visibility by adhering to the solid product.
- CThe cross is viewed through a constant depth of liquid.
- DThe cross is viewed over the largest possible area.
- EThe cross is viewed through a minimum depth of liquid.
Q5:
In a rate of reaction experiment between lumps of calcium carbonate and hydrochloric acid, what method or methods could you use to speed up the rate of reaction?
| A | B | C | D | E | |
|---|---|---|---|---|---|
| Method | Use larger lumps of calcium carbonate | Heat up the acid | Cool down the acid | Add a catalyst | Use a pestle and a mortar on the calcium carbonate |
- AB
- BA, B, and D
- CD
- DB, D, and E
- EB and D
Q6:
In a rate of reaction experiment between marble chips and hydrochloric acid, which of the following methods could you use to slow down the rate of reaction?
| A | B | C | D | E | |
|---|---|---|---|---|---|
| Method | Using powdered marble | Gently shaking the reaction vessel | Cooling down the acid | Using larger marble chips | Adding a catalyst |
- AB and D
- BC and D
- CB and E
- DA and C
- EC and E
Q7:
Sodium hypochlorite decomposes in light according to the equation shown: The rate of this photochemical reaction can be controlled by varying the intensity of light.
Which of the following is not an appropriate method of measuring this rate of reaction?
- AMeasuring the amount of oxygen produced over time
- BCounting the bubbles of oxygen produced over time
- CWeighing the mass of the solution over time
- DIncreasing the intensity of light over time
Q8:
For which of the following reactions would the apparatus in the diagram be unsuitable for measuring the rate of reaction?
- A
- B
- C
- D
- E
Q9:
When excess hydrochloric acid reacts with calcium carbonate, carbon dioxide is produced. Apart from measuring the change in mass of the calcium carbonate, which of the following could be measured to determine the rate?
- AThe intensity of light emitted over time
- BThe temperature of the reaction mixture over time
- CThe volume of gas produced over time
- DThe turbidity of the solution over time
- EThe color of the solution over time
Q10:
The diagram shows an experiment before and after the chemical reaction in the following equation takes place: Which of the following observations matches an increase in temperature of one or both of the reactants?
- AThe cross is obscured by the solid sulfur after more time.
- BThe cross is obscured by the solid sulfur after less time.
- CThe cross is obscured by the solid sulfur after a similar time.
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