Investigating the Thermal Decomposition Of Metal Carbonates
Aim: To investigate a range of metal carbonates and see if they
thermally decompose.
Thermal Decomposition
INVESTIGATION
[IMAGE]
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Written By Tauqir Sharif
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Research:
When a metal is thermally decomposed the bond between the metal and
its carbonate (carbon and oxygen) is removed and the carbonate is
released as carbon dioxide.
Metal Carbonate = Metal Oxide + Carbon Dioxide
Malachite is an ore of copper. It is made mostly of copper carbonate.
It can be crushed into a green powder. If this powder is heated it
changes colour. A new substance has been made. The new substance is a
black powder. This is called copper oxide. The copper carbonate has
been decomposed.
Copper oxide is made by thermal decomposition of copper carbonate.
Carbon dioxide is also made. The formula for this is:
Copper Carbonate = Copper Oxide + Carbon Dioxide
(CuCO3 = CuO + CO2)
The reactivity series determines how fast this reaction occurs. The
reactivity series is the order of metals in the periodic table. The
most reactive metals are placed at the top of the reactivity series.
The least reactive materials are placed at the bottom of the
reactivity series. From preliminary work that I have already done I
know that Potassium and sodium are the most reactive metals, and that
gold and platinum are the least reactive metals. To determine the
order of how reactive a metal is and where to place it in the
reactivity series you have to see how the metal reacts to:
Ø Oxygen (air)
Ø Water
Ø Acid
When metals are heated they react with oxygen in the air. As the metal
is heated it reacts with the oxygen to form an oxide. The most
reactive metals such as potassium and sodium burn brightly when they
are heated. The less reactive metals do not burn brightly, and take
longer to form their oxide.
During our investigation we first decided how much sodium bicarbonate we would be using. We decided on 11 grams which was about half of the crucible. We then used the bunsen burner to heat up the sodium bicarbonate. We heated the sodium bicarbonate expecting there to would be a chemical reaction and the atoms would be rearranged during thermal decomposition. We heated the sodium
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Compared with the accepted value of –601.8 kJ/mol Mg, our experimental error was 2.46%. Introduction In this investigation the change in enthalpy will be determined from the following equation: 2Mg + O2 ® 2MgO, but in an indirect manner. Magnesium metal burns on a bright, extremely hot flame to produce magnesium oxide. It would be difficult to measure the heat of the reaction since the reaction is rapid and occurs at a high temperature (LeMay et al, 1996).
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al. 1996). this dense produce is more thermally unbalanced than mulch or coal, mainly as of grass biomass. Little warming degrees and extensive residence eras will decrease the reactivity of the burn. On the other hand, great heating rates give to upsurge the reactivity of the subsequent char, creating it advanced appropriate for more thermal usage for example gasification or combustion (Hallgren, et. al. 1996).
CaCl2 + H2O + CO2
heat will stay in the cup and can only escape by rising to the surface
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Based on your experiments what is the formula of the colorless gas that is released when heating the malachite?
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· When I have collected my results I will place them in a table like
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