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Chemistry Practical Assignment - Copper carbonate - Lab Report Example

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Chemistry Practical Assignment - Copper carbonate

Take the given CuCO3 and weigh around 0.2 gm to the nearest to 0.01 gm of it in a test tube.
Carefully tight the cork fitted with a delivery tube on the mouth of the test tube and use sealant to close the leakage if any in the tube. Filled a water tray and fill the graduated cylinder with water, cover it and gently invert the graduated cylinder and bring it down so that its mouth of it is just beneath the water level in the filled tray. Ensure that there is no air bubbles at the time of putting graduated cylinder and it is fixed with the help of clamp. Put the delivery tube inside the mouth of the cylinder so that the air is passed to the inverted graduated cylinder. The experimental setup should look like as shown in figure-1 (Decomposition of copper carbonate, n.d.) and by putting the sealant material minimize the leakage from the corners and through the cork.
Now heat the copper carbonate gently with a burner (Thermal decomposition, 2007). The gas so formed is passed to the inverted graduated cylinder (Decomposition of copper carbonate a, n.d.). As soon the formation of gas bubbles stops, immediately take out the burner and keep the graduated cylinder perpendicular and take the meniscus reading and find out the volume of water displaced by the gas. Record the temperature of water and barometric pressure in the laboratory.
Repeat the experiment at least thrice and record the weight of copper carbonate taken for all the experiments and corresponding gas volumes.

Safety and Precautions: An irresponsible act can threaten our own safety and health in the laboratory (On carrying out experiment in the laboratory, n.d.) and therefore before conducting the experiment wear safety goggles and lab apron (Safety and Laboratory Rules, 1999). Avoid ingesting chemicals and use caution around open flames (Decomposition of copper carbonate, n.d.)

Calculations and Discussions: For evaluating both the equations, the mole concept is used (mole concept & Mole concept and mole conversion, nd). First using the following gas law the volume of gas at NTP has to be find out (Physical laws & Scaling, 2003).
P1 V1 P2V2
---- = ------- ----- (1)
T1 T2
As we have already collected the P1 (barometric pressure), V1( the gas volume ), T1 (the water temperature) and P2 is 760 mm of Hg and T2 is 273K and putting all values in above equation we will get, V2 the volume of gas at NTP.

Now according to equation 1, 2CuCO3(s) ----- Cu2O(s) + 2 CO2 (g) + O2 (g)
We will get 2 moles of carbon dioxide and 1/2 mole of oxygen from 2 mole of copper carbonate.
Now the molecular weight of CuCO3 = 123.5
The Weight of copper carbonate taken for study = 0.2 gm.
Therefore the mole of copper ca ...Show more

Summary

The important thing for finding the correct equation is that the volume of one mole of gas at NTP is 22.4 liter and using this equation we can back calculate the mole or mass of carbon dioxide formed from the copper carbonate used for the experiment (Determining the Correct Equation for the Decomposition of Copper Carbonate, 2003) and hence find out the correctness of the eauation provided.
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