• 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
5. 5
5
6. 6
6
7. 7
7
8. 8
8
9. 9
9
10. 10
10
11. 11
11
12. 12
12
13. 13
13
14. 14
14
15. 15
15
16. 16
16

# Look at two variables that affect at the speed of the reactions between Marble Chips (CaCO3) and Hydrochloric Acid (HCl).

Extracts from this document...

Introduction

In this piece of coursework I am going to look at two variables that affect at the speed of the reactions between Marble Chips (CaCO3) and Hydrochloric Acid (HCl). I will use four different states of division of the marble chips. These will be: * Large chips * Medium chips * Small chips * Powder I will also vary the concentration of my Hydrochloric acid. * 2.5 Molar * 2.0 Molar * 1.5 Molar * 1.0 Molar * 0.5 Molar In any reaction a solid is needed, our solid is Marble Chips. EQUIPTMENT: * Beakers (250ml) * Measuring cylinder (50cm3) * Bungs * Thermometer (00C-110oC) * Electronic Scales (0.00g) * Weighing boats * Boiling tubes (50cm3) * Marble chips (Small, Medium and Large) * Hydrochloric acid (2.5 - 0.5 Molar) From this reaction, Carbon Dioxide is produced, and it is the collection of this gas that will measure the reaction for us. I predict that, " the more concentrated the acid, the quicker the reaction will be." Also " the larger the chips, the longer the reaction will take." I think this because a reaction occurs when particles collide. This process is based on random particle movement. ...read more.

Middle

Because of the fact that the marble chips come with a thin layer of powder on the outside, we have decided to leave the reaction for thirty seconds at the beginning before we start collecting the Carbon Dioxide. After the thirty seconds, we placed a boiling tube (50cm3) on top of the glass tube coming from the conical flask and timed to see how long it takes to fill the tube completely with the Carbon Dioxide. We will also measure the temperature of the room, because it may be carried out on different days so the temperature could have changed. This temperature change could affect our results by many seconds. I believe that my prediction that " the more concentrated the acid, the quicker the reaction will be,'' will be proven correct because stronger acids come with more severe warnings on them, thus must be more corrosive. The more corrosive an acid is the faster it should make this reaction happen. The equation is CaCO3 + 2HCl CaCl2 + H2O + CO2 Firstly we tested the different chip sizes and came up with these results. Time in Second Size of Chips Time 1 Time 2 Average Rate 1/time in seconds S 14 13 13.5 0.74 M 23 22 22.5 0.04 L 26 ...read more.

Conclusion

All my readings were repeated and an average was taken. If there were an anomalous result they were re-tested and changed accordingly. My equipment was kept the same the whole way thought the experiment so the only things that were changing were my variables. This means that my experiment was a fair test thus the results are as reliable as they could be. After doing my experiment and analysing my findings I can now say that there are two clear conclusions The more concentrated an acid is the faster it will react The larger the surface area of a reactant the faster the reaction will be Because of the fact that my experiment met my expectations and the exportations of basic science, I would say that my experiment has nothing that needs changing. I am very happy with the way my experiment went and with my method. However it would have been nice to get all the results done in the one day, because there could have been different factors that could potentially have affected my work, e.g. using different apparatus, the apparatus I am using may have other chemicals left in it, or there could have been a small temperature rise, that was not noticed on the thermometer, these are all small things that could affect my results in a big way. ...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. ## In this investigation we are going to measure the rate of reaction of marble ...

3 star(s)

64 29 33 31 31 29-33 460 65 33 37 34 35 33-37 480 68 33 37 36 35 33-37 500 69 33 37 36 35 33-37 520 72 33 37 37 36 33-37 540 75 37 37 37 37 37 560 75 37 37 37 37 37 580 75

2. ## Investigate how concentration of hydrochloric acid (HCL) affects its reaction with calcium carbonate (CaCO3).

I would still not be able to take measurements in my real experiment if I chose these measurements, because it is still too fast. I decided to lower the mass of the chips to 1.4g, increase the size of the chip to large and lower the molar to 2.

1. ## How does changing the concentration of the Hydrochloric acid affect it reactions with Magnesium?

had just enough for 1 mole of magnesium to react with two of HCl. To get a fair reaction we had to keep the amount of magnesium the same and the temperature. We used 0.1g of magnesium. RESULTS Temperature From this graph you can see that if we do increase

2. ## To investigate the factors which affect the rate of reaction between marble chips and ...

min Average results Formula for working out: Average Rate of reaction == total volume of CO2 in cm3 ______________________________ Total time for reaction Size of chips Total volume of CO2 (g) (cm3) Total time for reaction Average Rate of reaction Medium (9-12mm)

1. ## An investigation to find out how the concentration of acid affects the rate of ...

can also have an impact. Safety Safety is very important in this, and any, experiment so I will wear safety specs when carrying it out to protect my eyes from becoming damaged by the acid. I will also wear an apron to protect my clothes from the same.

2. ## An Experiment to investigate whether the concentration of HCl affects the rate of reaction ...

In a reaction between two gaseous substances A&B a molecule of A must collide with B for the reaction to proceed but in a concentrated solution there will be a higher percent of reactants which will have no more energy.

1. ## Exothermic and endothermic reactions

Each hydrocarbon has a different boiling point. This is handy because we use the different boiling points to separate them. There is a link between how many carbon atoms a hydrocarbon has and its boiling point. For example, look at the four hydrocarbons in the table: Name of hydrocarbon Formula

2. ## How does the concentration of HCl affect the rate of reaction with CaCO3?

* Pipette ? we used a pipette to put hydrochloric acid into the 10ml measuring cylinder because it helped us put the hydrochloric acid exactly to the 10 ml. * 0-10 ml measuring cylinder ? we used this because it eliminated any chances of us putting anything higher than ten

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