To monitor the rate of production of oxygen from hydrogen peroxide using manganese dioxide as a catalyst Flashcards Preview

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Flashcards in To monitor the rate of production of oxygen from hydrogen peroxide using manganese dioxide as a catalyst Deck (13)
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1
Q

How can the reaction could be started at a known time?

A

Add catalyst, stopper and start clock

2
Q

How is the gas produced collected?

A

Delivery tube is connected to gas collection system

3
Q

How is the gas measured

A

Inverted graduated cylinder

4
Q

Describe the appearance of the manganese dioxide before use

A

A black powdery solid

5
Q

Name the products of the decomposition of hydrogen peroxide

A

Water and Oxygen

6
Q

The hydrogen peroxide is said to be ‘20 volume’. What does this mean?

A

That a certain volume of hydrogen peroxide would give off 20 times that volume when it decomposes

7
Q

What property of the gas allows collection under water?

A

The fact that oxygen is only sparingly soluble in water allows it to be collected under water

8
Q

Describe the appearance of the manganese dioxide at the end of the reaction. Would you expect to see a change in appearance and explain

A

Black powdery solid

No, because the manganese dioxide acts as a catalyst and a catalyst is usually unchanged at the end of the reaction

9
Q

Give one every day use of manganese dioxide

A

Manufacture of ‘dry’ batteries

10
Q

Give a balanced equation for this reaction

A

H2O2 -> H2O + 1/2 O2

11
Q

What type of catalysis was involved in these reactions?

A

Hetergenous

12
Q

When the graph is plotted of the volume of gas produced versus time explain why the graph is steepest at the beginning

A

Highest concentration - more collisions

13
Q

Calculate the total mass of gas produced in this experiment when its 78cm^3 volume

A

78 ÷ 24000 = 0.00325 mol × 32 = 0.104