• 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

# Experiment to investigate the effect of the concentration on the rate of reaction

Extracts from this document...

Introduction

Experiment to investigate the effect of the concentration on the rate of reaction Introduction: - Rate of reaction is the measure of the length of time taken for a reaction to occur. Factors that affect the rate of reaction are (This is the general view, check hypothesis):- i. Temperature of the Solution ii. Surface Area of the Solid iii. Concentration of the Solution Rate of reaction can be measured using several techniques. These involve measuring the rate of which the product is made or the rate at which a reaction is used up. The balanced chemical equation and word equation reaction between Hydrochloric Acid and Calcium Carbonate is shown below:- The reaction: - Hydrochloric + Calcium Carbon + Calcium + Water Acid Carbonate Dioxide Carbonate 2HCl (aq) + CaCO3 (s) CO2 (g) + CaCl2 (aq) + H2O (l) It can be seen from the equation that this reaction produces CO2 gas. Therefore, it is possible to measure the rate of reaction by measuring the volume of the gas produced within a certain length of time. Aim: - To investigate the effect of changing the concentration of the Hydrochloric Acid on the rate of reaction between Hydrochloric Acid and Calcium Carbonate in the form of marble chips. Hypothesis: - What was kept constant: - 1. Temperature of the Acid 2. Concentration of Hydrochloric Acid 3. The total weight of the Marble Chips 4. Volume of the Hydrochloric Acid Preliminary Experiment: - This involved determine the size of the marble chips (calcium carbonate) to use in the experiment. Equipment used to determine this: - Conical Flask (250 ml) Measuring Cylinder (250 ml) Gas Syringe (Fitted with bung) Hydrochloric Acid Concentrations (1M, 2M, 3M, 4M) Delivery Tube Marble Chips in grams (small, medium and large) Goggles Timer Water Bath + thermometer (25?C) Digital Balance Diagram 1: - Method: - 1. Wear goggles for safety 2. Temperature kept constant by placing Hydrochloric Acid in a water bath (this was constant at temperature 25�C) ...read more.

Middle

* To measure the time for the results in how much gas is given off to how long it takes to fill the Gas Syringe. This is to get the results and plot on a graph to show the accurate results * To measure how long it takes to give off 100 cm3 of CO2 gas. To get the results on the table and on the graph. Results for the main experiment: - Volume of CO2 (g) produced (cm3) from the reaction between different concentrations of Hydrochloric Acid and small sized marble chips. Volume of CO2 produced (cm3) Volume of CO2 produced (cm3) Time (sec) 1M 1st 1M 2nd 1M 3rd Average Time (sec) 2M 1st 2M 2nd 3M 3rd Average 5 6 4 5 5 5 12 10 7 11.7 10 8 6 7 7 10 35 30 22 29 15 11 10 10 10.3 15 50 45 35 43.3 20 14 15 14 14.3 20 74 58 56 62.6 25 18 21 17 18.6 25 100 80 77 85.6 30 23 28 22 24.6 30 99 86 92.5 35 26 36 17 29.6 35 100 100 40 35 44 34 37.6 45 38 55 37 43.3 50 42 63 43 49.3 55 47 75 50 57.3 60 58 86 58 67.3 65 68 100 66 78 70 75 75 75 75 78 85 81.5 80 85 91 88 Volume of CO2 produced (cm3) Volume of CO2 produced (cm3) Time (sec) 3M 1st 3M 2nd 3M 3rd Average Time (sec) 4M 1st 4M 2nd 4M 3rd Average 5 28 21 20 23 5 45 40 42 42.3 10 45 43 45 44.3 10 72 70 71 71 15 81 71 81 77.6 15 95 92 93 93.3 20 100 100 100 100 20 100 100 100 100 Interpretation of results 1. The volume of CO2 (g) produced (measured in cm3) increased with the increase of time (seconds) ...read more.

Conclusion

Further investigations: - 1. Look at actual mathematical relationship in further detail between Hydrochloric acid and the rate of reaction by using different concentrations. E.g. 0.25M & 0.5M 0.5M & 1M 2. Look at actual mathematical relationship between mass of CaCO3 and rate of reaction. (1 and 2 would allow rate of reaction to be formulated) 3. Look at the effect of the factors on rate e.g. surface area of chips or the addition of catalysts. Appendix for the main experiment: - Volume of CO2 (g) produced (cm3) from the reaction between different concentrations of Hydrochloric Acid and small sized marble chips. Volume of CO2 produced (cm3) Volume of CO2 produced (cm3) Time (sec) 1M 1st 1M 2nd 1M 3rd Average Time (sec) 2M 1st 2M 2nd 3M 3rd Average 5 6 4 5 (6+4+5)/3=5 5 12 10 7 (12+10+7)/3=11.7 10 8 6 7 (8+6+7)/3=7 10 35 30 22 (35+30+22)/3=29 15 11 10 10 (11+10+10)/3=10.3 15 50 45 35 (50+45+35)/3=43.3 20 14 15 14 (14+15+14)/3=14.3 20 74 58 56 (74+58+56)/3=62.6 25 18 21 17 (18+21+17)/3=18.6 25 100 80 77 (100+80+77)/3=85.6 30 23 28 22 (23+28+22)/3=24.6 30 99 86 (99+86)/2=92.5 35 26 36 17 (26+36+17)/3=29.6 35 100 100/1=100 40 35 44 34 (35+44+34)/3=37.6 45 38 55 37 (38+55+37)/3=43.3 50 42 63 43 (42+63+43)/3=49.3 55 47 75 50 (47+75+50)/3=57.3 60 58 86 58 (58+86+58)/3=67.3 65 68 100 66 (68+100+66)/3=78 70 75 75 (75+75)/2=75 75 78 85 (78+85)/3=81.5 80 85 91 (85+91)/3=88 Volume of CO2 produced (cm3) Volume of CO2 produced (cm3) Time (sec) 3M 1st 3M 2nd 3M 3rd Average Time (sec) 4M 1st 4M 2nd 4M 3rd Average 5 28 21 20 (28+21+20)/3=23 5 45 40 42 (45+40+42)/3=42.3 10 45 43 45 (45+43+45)/3=44.3 10 72 70 71 (72+70+71)/3=71 15 81 71 81 (81+71+81)/3=77.6 15 95 92 93 (95+92+93)/3=93.3 20 100 100 100 (100+100+100)/3=100 20 100 100 100 (100+100+100)/3=100 This is another way to show the results given but the Bar Graph would be complicated to look at. The Line Graph would be easier to retrieve data from Time against concentration. ...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. ## Marble Chips and Hydrochloric Acid.

4 star(s)

Concentration 0 0.25 0.5 1.0 1.5 2.0 Rate 0 0.22cm�/sec 0.44�/sec 0.98�/sec 1.49�/sec 1.99�/sec A pattern has occurred as to how much Carbon dioxide is released. 1 mole of acid released 0.98cm� of CO and 2 moles released 1.99cm� per second.

2. ## The Effect of Concentration on the Rate of Reaction between Hydrochloric Acid and Calcium ...

3 star(s)

This means activation energy will not have an effect on this experiment. - Catalyst- A catalyst will lower the activation energy and makes more successful collisions, by weakening the bonds and increasing the rate of reaction. When the activation rate is lower not much energy is needed to make the reaction successful.

1. ## In this investigation we are going to measure the rate of reaction of marble ...

3 star(s)

being greater than the other two; consequently this result will be discarded and not used in calculating averages. Results for 1M HCl: Medium Marble (CaCO3) 1M HCl Volume of CO2 /cm� Time (s) Test 1 Test 2 Test 3 Test 4 Average Range 0 0 0 0 0 0 0

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

I have explained each factor listed in detail in my Evaluation. Evaluation After doing my experiment I can say that it went reasonably well. This is because the results I got from the experiment were good enough to support my hypothesis that I made at the start which was: "I believe that as the concentration of hydrochloric acid (HCL)

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

An increased concentration means more particles. This increases the chance of a collision and, hence, an increased rate of reaction. Low pressure or concentration High pressure or concentration Prediction: (activation energy and collision theory) In Brief: Using the scientific knowledge, stated above, I predict the rate of reaction increases when the surface area of a solid reactant is increased.

2. ## An Experiment To Investigate The Rate Of Reaction Between Marble Chips And Hydrochloric Acid.

0 20 3 0.0 0.00 0.00 Reactions cannot occur by simply putting two substances together. The substances must be reactant with each other, the particles must collide with each other, and they must collide with enough energy to break the bonds that keep the particles together.

1. ## Investigation into the Effect Concentration has on Rate of Reaction.

Distilled Water I am using distilled water in order that it is neither acidic nor alkaline, and therefore does not affect the reaction. SAFETY This is an experiment involving acid, which can be highly dangerous if it comes in contact with skin or eyes.

2. ## Investigating the rate of reaction between hydrochloric acid and calcium carbonate

is a greater chance of a reaction happening as reactions happen when ions collide. All my lines of best fit go through the origin as after no time no reaction has happened. All of my lines of best fit are more or less directly proportional so when you double the amount of time the amount of gas released also doubles.

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