Calcium Carbonate + Hydrochloric Acid -> Calcium Chloride + Water + Carbon Dioxide

September 24, 2017 September 1st, 2019 Free Essays Online for College Students

CaCO3 + 2HCl -> CaCl 2 + H2O + CO2

Aim

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Investigate factors affecting rate of reaction between calcium carbonate and hydrochloric acid.

Method & Diagram

Fill measuring cylinder with water

Half fill water basin with water

Invert measuring cylinder whilst covering open end with hand

Submerge measuring cylinder (End with hand on)

Put 25ml of acid into the conicle flask

Have 2.0g of marble chips ready

Put end of pipe into submerged conicle flask

Prepare to start stopwatch

Put marble chips in with acid & put bung on conicle flask whilst starting stopwatch

Every 30s starting from 0s take a measurement of how much air there is in measuring cylinder (cm3)

When you have done this with the first concentration of acid clean out the conicle flask and refill the measuring cylinder & repeat experiment with next concentration of acid.

Equipment

* Water

* Conicle Flask

* Bung

* Marble chips

* Water Basin

* Tube

* Acid amounts (0.25M, 0.5M, 1.0M, 1.5M, 2.0M)

* Timer

Vairiables

Concentration of acid -> higher the concentration faster the reaction

Mass of limestone – (Which is not changed other than test specs)

Surface area of limestone – Greater the surface area -> faster rate of reaction

Temperature – Increasing the temp -> increases the reaction rate

Theory

The concentration of acid has a major effect on the results. For our experiment we used 25ml of acid (All of the concentrations used the same amount) 0.25M, 0.5M, 1.0M, 1.5M, 2.0M. ‘M’ Means molar which is how the strength of acid is measured.

The stronger the concentration of acid used will effect the amount of gas produced, the more acid used – the more gas created & visa versa.

Prediction

I predict the more gas made will be dependent on how much acid is added.

Safety

* Use goggle eye protection

* Rinse acid contacted area with water & seek help

Results

Experiment 1

0.25M

0.5M

1.0M

1.5M

2.0M

0

0

0

0

0

0

30

2

4

10

20

30

60

4

6

24

50

64

90

8

8

42

80

114

120

10

14

60

106

146

150

12

16

75

130

178

180

13

18

90

152

204

210

15

30

115

174

222

240

16

42

130

194

244

270

18

52

142

210

265

300

20

58

172

224

277

Experiment 2

0.25M

0.5M

1.0M

1.5M

2.0M

0

0

0

0

0

0

30

3

4

10

15

33

60

5

7

22

40

67

90

7

14

34

75

116

120

9

18

54

100

145

150

11

25

75

125

179

180

12

30

90

144

205

210

14

39

100

160

225

240

16

45

115

180

242

270

17

55

128

196

269

300

20

64

141

208

274

Averages Table

0.25M

0.5M

1.0M

1.5M

2.0M

0

0

0

0

0

0

30

2.5

4

10

17.5

31.5

60

4.5

6.5

23

45

65.5

90

7.5

11

46

77.5

115

120

9.5

16

57

103

145.5

150

11.5

20.5

75

127.5

178.5

180

12.5

24

90

148

204.5

210

14.5

34.5

107.5

167

224

240

16

43.5

122.5

187

243

270

17.5

53.5

135

203

267

300

20

61

156.5

216

275

Conclusion

My results have shown that when i use a stronger acid the rate of reaction between calcium carbonate and hydrochloric acid increases because, there is more contact between particles of acid and particles of calcium carbonate. There is a definate partern to both my graphs and results and this is that the stronger the acid the quicker carbon dioxide was produced. This is shown of the graphs by a steadily increasing line.

This proves my prediction to be correct, because I predicted that a stronger acid would give more carbon dioxide quicker than a weaker acid and this was true. 2.0M acid was so fast compared to 0.5M acid because in 2.0M acid there is a higher concentration of particles of acid so there is more chance of a collision between acid particles and calcium carbonate particles. In 0.5M acid it was so slow because there is a quater of the amount of acid particles in 2.0M acid. I can draw a labelled diagram which shows particles of acid colliding with marble chips and making gas and I can use this to explain what I found out in my results.

Evaluation

I cannot think of a better way of doing the experiment or collecting more accurate results except than using more detailed measuring cylinder’s. I do think that taking averages helps because it gives an average result which means that it can be more accurate than lots of individual results. The main difficulties in doing this experiment I think were taking results accurately.

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