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):
1

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

Add catalyst, stopper and start clock

2

How is the gas produced collected?

Delivery tube is connected to gas collection system

3

How is the gas measured

Inverted graduated cylinder

4

Describe the appearance of the manganese dioxide before use

A black powdery solid

5

Name the products of the decomposition of hydrogen peroxide

Water and Oxygen

6

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

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

7

What property of the gas allows collection under water?

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

8

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

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

Give one every day use of manganese dioxide

Manufacture of 'dry' batteries

10

Give a balanced equation for this reaction

H2O2 -> H2O + 1/2 O2

11

What type of catalysis was involved in these reactions?

Hetergenous

12

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

Highest concentration - more collisions

13

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

78 ÷ 24000 = 0.00325 mol × 32 = 0.104