• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month
Page
1. 1
1
2. 2
2
3. 3
3
4. 4
4

# To Find Out How Much Surface Area Affects the Rate of a Reaction Between a Potassium Tablet (K2co3) and Hydrochloric Acid (Hcl).

Extracts from this document...

Introduction

The Rate of Reaction Equation K2CO3 + HCl KCl + H2O + CO2 Aim The aim of the experiment is to find out how much surface area affects the rate of a reaction between a potassium tablet (K2CO3) and hydrochloric acid (HCl). Variables The variables for this experiment include: ? The temperature of the HCl. ? The concentration of the HCl. ? The surface area of the K2CO3. For this experiment I will be testing the surface area. Prediction I think that as the surface area of the surface area of the K2CO3 decreases the rate of the reaction will increase. ...read more.

Middle

Repeat this experiment with exactly the same quantities. Then repeat this (including the repeat with the same quantities) cutting the K2CO3 into 1/2, 1/4 and 1/8. Results Time Taken (mins) 1st 0:30 1:00 1:30 2:00 2:30 3:00 Attempt 1 34 50 80 90 94 95 (amount 1/2 34 58 76 80 82 --- of gas 1/4 39 50 72 75 --- --- Produced ml) 1/8 62 73 80 --- --- --- ----------- --------- --------- --------- --------- --------- --------- ----------- 2nd 1 63 84 100 105 --- --- Attempt 1/2 62 81 82 90 100 --- 1/4 57 82 99 102 102 1/2 --- 1/8 34 72 79 80 --- --- Conclusion The results should have concluded my theory that as the size of the K2CO3 decreased the rate of the reaction should have increased. ...read more.

Conclusion

This is shown in the diagrams below: These diagrams are showing that because the K2CO3 particles are more dispersed in the right diagram than the left and so there is more chance of a HCl particle hitting a K2CO3 particle. Evaluation This experiment was badly done by me. This is partly because I was working on my own (there are no other reasons that I can think of). I think I could have taken more time on it and better care. The second set of results reflects the value of the results better than the first set of results. In all of the tests that I did there were three ominous results and this have been highlighted on the graphs. Overall the experiment did not turn out the way that it should have. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

## Found what you're looking for?

• Start learning 29% faster today
• 150,000+ documents available
• Just £6.99 a month

Not the one? Search for your essay title...
• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

# Related GCSE Patterns of Behaviour essays

1. ## An investigation into how surface area affects the rate of reaction.

At a high concentration, there are more acid particles in a certain volume. This means there is a higher chance of a collision because there are more acid particles. As there are more collisions, the rate of the reaction will increase.

2. ## An investigation into how surface area affects the rate of reaction

This happens because by increasing the surface area we are also increasing the rate of collisions between the particles. When there is more of the reactant to react with the reaction speeds up. Therefore, my hypothesis is: the reaction will be faster when using small chips, so the gas will

1. ## Investigation to find out how particle size affects the reaction rate.

To do this I will use the same volume and concentration of hydrochloric acid throughout and will also keep the mass of the particle sizes the same throughout. I will also use the same scales while doing my experiment so that no faulty mass is calculated making my experiment unfair

2. ## An Investigation into the effect of concetration on the Rate of Reaction Between Potassium ...

This is reacted with the 10cm3 of iodide and 0.03ml starch and the reaction was timed until the cross disappeared and again was repeated three times and an average was taken. This same process was repeated, by adding to the 10cm3, 10ml, 15ml, 20ml, 25ml, 30ml, 35ml, 40ml, 45ml, 50ml and 55ml of distilled water each time.

• Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to