<body><script type="text/javascript"> function setAttributeOnload(object, attribute, val) { if(window.addEventListener) { window.addEventListener('load', function(){ object[attribute] = val; }, false); } else { window.attachEvent('onload', function(){ object[attribute] = val; }); } } </script> <div id="navbar-iframe-container"></div> <script type="text/javascript" src="https://apis.google.com/js/platform.js"></script> <script type="text/javascript"> gapi.load("gapi.iframes:gapi.iframes.style.bubble", function() { if (gapi.iframes && gapi.iframes.getContext) { gapi.iframes.getContext().openChild({ url: 'https://www.blogger.com/navbar/4496823545544314871?origin\x3dhttps://chemistryproject2012.blogspot.com', where: document.getElementById("navbar-iframe-container"), id: "navbar-iframe" }); } }); </script>



profile entries tagboard links
CHEMISTRY
Group Members: WanQin, Delia, PeiPei & Marie

Hey , You are welcoming here .
This is our chemistry project this year (2012).
Our topic is on heating of metal carbonates,
we hope that you will learn something from here.

Friday, 7 September 2012, 00:49
Conclusion

Conclusion

Based on all the various videos, with the help of the internet and support from the Chemistry textbook, we conclude that  the ability for carbonate to decompose is related to the position of metals in the reactivity series. The more reactive metal is more stable to heat thus it will not decomposed upon heating. Metal-carbonate below sodium decomposed upon heating to form metal oxide and carbon dioxide with the exception of silver carbonate which will decompose to form silver and carbon dioxide.

, 00:14
Videos of Experiments

VIDEOS
credits: youtube

 Heating of Lead(II) Carbonate



















Heating of Copper(II) Carbonate



















Heating of Zinc Carbonate

Thursday, 6 September 2012, 23:30
Experiments & Equations


EXPERIMENTS
Apparatus set-up
1. Add a large spatula measure of the carbonate in a test-tube.
2. Fit a delivery tube into the test tube and then clamp the test-tube so that the delivery tube dips into a second test-tube containing 2-3 cm3 limewater.
3. Heat the solid slowly at first, then more strongly.
4. Repeat the experiment with the other metal carbonates given, and write down your observations for each of the reaction.

 Carbonate
 Colour (before being heated)
 Colour (after being heated)
 Gas given out
 Potassium Carbonate
 white
 white 
 none
 Sodium Carbonate
 white
 white
 none
 Zinc Carbonate
White
 yellow then white when cooled
 Carbon dioxide
 Lead Carbonate
 white
 yellow
 Carbon dioxide
 Copper Carbonate
 green
 black
 Carbon dioxide


Chemical Equations:
  • K2CO3 --> no reaction
  • Na2CO3 --> no reaction
  • CaCO3 --> CaO + CO2
  • MgCO3 --> MgO + CO2
  • ZnCO3 --> ZnO + CO2
  • FeCO3 --> FeO + CO2
  • PbCO3 --> PbO + CO2
  • CuCO3 --> CuO + CO2
  • Ag2CO3 --> Ag2O + CO2

, 23:03
Heat on Metal Carbonates

Thermal decomposition
Metal carbonates such as calcium carbonate break down when heated strongly. This is called thermal decomposition. It is a endothermic reaction as heat is required to break chemical bonds in the compound undergoing decomposition.
calcium carbonate right facing arrow with heat calcium oxide + carbon dioxide
CaCO3right facing arrow with heat CaO + CO2

Some compound are more difficult to decompose by heating than others. This mean that these compounds are more stable to heat than others.Thermal stability of metal carbonate is in relation to the position  of the metal in the reactivity series. The more reactive metals-carbonate are harder to decompose.Metal-carbonate after sodium form metal oxide and carbon dioxide upon heating all in the exception of silver carbonate which decompose into silver and carbon dioxide upon heating. 



 Metal Carbonate
 Observation
 Potassium Carbonate, K2CO3
 no reaction
 Sodium Carbonate, Na2CO3
 no reaction
 Calcium Carbonate CaCO3
 decompose into metal oxide and carbon dioxide upon heating
 Magnesium Carbonate MgCO3
 decompose into metal oxide and carbon dioxide upon heating
 Zinc carbonate ZnCO3
 decompose into metal oxide and carbon dioxide upon heating
 Iron (ll) carbonate FeCO3
 decompose into metal oxide and carbon dioxide upon heating
 Lead (II) carbonate PbCO3
 decompose into metal oxide and carbon dioxide upon heating
 Copper(II) carbonate CuCO3
 decompose into metal oxide and carbon dioxide upon heating
 Silver carbonate Ag2CO3
 decomposes into silver, oxygen gas & carbon dioxide upon heating




credits: Chemistry textbook
              http://www.bbc.co.uk/schools/gcsebitesize/science/aqa_pre_2011/rocks/limestonerev1.shtml
                   http://en.wikipedia.org/wiki/Thermal_decomposition