• 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

# Does temperature affect the reaction rate between chalk powder and hydrochloric acid.

Extracts from this document...

Introduction

In this experiment, I am going to see if temperature affects the reaction rate between chalk powder and hydrochloric acid by timing how long it takes for the chalk powder to dissolve in the acid! There are many variables that could be used in this experiment! They are: - * Concentration of acid * Surface area of chalk Powder * Amount of chalk 0.1g * Volume of hydrochloric acid 10ml * Temperature of acid The variable I am going to change is Temperature of acid. This is because it is the easiest to do! All the rest I will have to keep the same to make it a fair test. I predict that if you increase the temperature of the acid in the experiment, it will speed up the reaction time the faster the reaction rate. This is due to the kinetic theory. The more heat that is given to the acid, the faster the particles move. ...read more.

Middle

I will then measure the chalk keeping the same amount of powdered chalk! I have to put the piece of paper on first and then put the chalk on top, so when I do put the piece of paper on I will have to put the scales back to zero because the paper has a mass so it will effect my results. I have to do this to make it a fair test. The next thing I have to do is measure the hydrochloric acid out accurately with a measuring cylinder. I will the heat it in the water bath to get my desired temperature. I will then set the stop clock to zero and put the 0.1g of chalk in the heated acid! I will the start the stop clock when the reaction has stopped. I will repeat this experiment 3 times and increase the temperature by 10oC each time. This is to make my results reliable because one of them might have gone wrong! These are my results. ...read more.

Conclusion

They are average results. This graph had a smooth line but my first result took a lot more time than all the others. There might have been a lump in the chalk but all the times I tried it the results were around the same amount of time! The experiment went quite well. There weren't any odd results and nothing went wrong. Although I have some ideas which may gain an even more accurate reading. Firstly, there could have been some lumps in the chalk. That may be why the first result took so long! Secondly, there might have been a slight delay in the time we started the stop clock and when we put the chalk into the acid. It wouldn't have affected my results by much but that was a thing I could improve. There are many possible extensions to this experiment. I could try to use other substances and react them with hydrochloric acid. I could also try different acids and see what happens. All these could help me with my knowledge on reaction rates. By Richard Griffiths 10R ...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 Aqueous Chemistry 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 Aqueous Chemistry essays

1. ## To investigate the effect of temperature on the rate of reaction

4 star(s)

When the solution was at 70oC, the rate of reaction was 2.75 Vm/sec-1 and when the solution was 40oC, the rate was 1.1Vm/sec-1. This was because when the temperature was higher, particles had more kinetic energy, collided more and had more energy than that of what is needed to activate the reaction.

2. ## The Rates of Reaction of Metals with Acid.

Seen below are the three molecular models of acid. The reason why Sulphuric acid has such a low activation is due to the pie bonds. These pie bonds attract the electrons toward them from the O - H Sigma bond to form a cloud nearer the sulphur molecule. As the pie bonds are shorter and closer to the sulphur, it makes them stronger and so attracts these electrons.

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