• 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

# Thermal decomposition of Copper Carbonate (CuCo3).

Extracts from this document...

Introduction

08 December 2003 Lehaz m kaker Thermal decomposition of Copper Carbonate (CuCo3) Plan: Introduction: In this experiment I'm going to identify the correct balanced stiochiometric chemical equation for the decomposition of the copper carbonate from the volume of carbon dioxide produced. Green powder of the copper carbonate is decomposed by heat. Two different equations are possible for this reaction. Equation 1: 2 CuCo3(s) Cu2O(s) + 2Co2(g) + O2 (g) Equation 2: CuCo3(s) Cuo(s) + Co2(g) We are to find the accurate equation for the decomposition of the CuCo3 from the volume of carbon dioxide produced from the known amount of copper carbonate decomposed. Safety: 1: Eye protection and lab coat must be worn. 2: Keep the bags and coat and other stuff away from the experimental area, as this is a flame involve practical. May cause trip falls. ...read more.

Middle

(High flame is not needed as the copper carbonate burns on a low blue flame) As the Carbon dioxide is collected in cylinder the water is replaced from graduation cylinder. When the CuCo3 decomposed completely the bubbles stop. 7) Waite until the temperature of carbon dioxide cool down to room temperature, because the volume of gas changes with temperature and pressure. Measure the temperature in water as it is replaced with Co2 gas. But water react with carbon dioxide while we wait, which will affect the volume of Co2 gas. To prevent this reaction we have to saturate the water with carbon dioxide gas by passing the Co2 through water. 8) After the Co2 cooled down to room temperature read the meniscus of water carefully and record the volume of carbon dioxide collected in the graduation cylinder. Result: Mass of sample (CuCo3)+sample-container = ...g Mass of sample residues+sample-container =...g Mass of sample (CuCo3) ...read more.

Conclusion

of O2 =...g In equation 2: The ratio between CuCo3 to Co2 is 1:1, so No of moles of CuCo3 = No of mole of Co2 Or 1 mole of Co2 = 24dm3 at 25C and 1 atm pressure X moles of Co2 = volume of Co2 produced at 25C and 1 atm pressure No of mole of Co2 = volume of Co2 produced in dm3 / 24dm3 Molar mass of Co2 = 44g Mass of Co2 = no of moles of Co2 X 44 = ...g Mass of Co2 =...g When we performed the above calculation now we can deduce the no of moles and mass of the product formed from the decomposition of the copper carbonate. Conclusion: The correct balanced stiochiometric equation for the thermal decomposition of copper carbonate can be deduce while carry out the experiment and measure the correct amount of CuCo3 decomposed and the volume of carbon dioxide produced by applying the above calculation. ...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 Classifying Materials 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 Classifying Materials essays

1. ## In this CDA I will write about how plastic bags are made, why plastic ...

More trees would be chopped down and therefore less biodiversity and more habitat loss for animals. Plastic bags are also convenient if you want to take some packaging just in case, as it scrunches into a small ball. Although some plastic bags may be weak, from my investigation I found

2. ## Copper has two oxides, Cu2O, and CuO. Copper carbonate, CuCO3 decomposes on heating to ...

24.291... = 24.29cm3 (2dp) Equation 2: CuCO3 (s) (r) CuO (s) + CO2 (g) 1 mole CuCO3 (r) 1 mole gas, ie 24dm3 123.5g CuCO3 (r)24000cm3 0.1g CuCO3 (r) 19.433... =19.43cm3 (2dp) When an element like copper can form two oxides, which one forms is based on the stability of the compound formed.

1. ## To investigate the thermal decomposition of copper carbonate and try to prove that the ...

= CuO Carbon Dioxide = CO2 copper + oxygen carbon + oxygen(x 2) 64 + 16 12 + 16(x 2) 80 44 80 + 44 = 124 The atomic numbers of copper oxide and carbon dioxide add up to the same atomic number as copper carbonate, which also proves that

2. ## Calcium carbonate reacts with dilute hydrochloric acid according to the equation below

In this case, the experiment has shown, that although there are some anomalous results, the reaction between calcium carbonate and hydrochloric acid is directly proportional to the concentration of acid. This shows that it is a first order reaction. Evaluation The results that I have collected are fairly accurate and

1. ## Thermal Decomposition of copper carbonate

Copper (II) compounds are by far the most common - they are called "cupric". Copper (I) compounds - "cuprous" compounds are far less common. Copper atoms most readily go to oxidation state +2, by a variety of reactions. Cupric compounds are unstable in the presence of water, so must either be insoluble or form complexes with other molecules.

2. ## The role of mass customization and postponement in global logistics

In the wake of growing competition, even government controlled firms have started to practice customisation in limited ways. Cooptex, the Cooperative textile firm of Tamil Nadu, Government has introduced recently the free selection of design, pattern etc. for the silk and cotton sarees by the consumers through computers which can be produced and delivered in a definite period.

1. ## Decomposition of copper carbonate - proving one of two equations.

The experiment can then be carried out, and the volume of gas produced compared with the predictions for each equation. Whichever equation best predicts the volume given off is therefore shown to be the correct one. Equation 1: 2CuCO3 (s) � Cu2O (s) + 2CO2 (g) + 1/2 O2 (g)

2. ## Bonding Practical

To test for this you just need a nickel tray or something to put the substance on and a Bunsen burner. A stopwatch could also be used to record the time it takes to melt the substance. Is it dense This follows on from the previous experiment.

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