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
Purpose: To identify the mystery powder based on its physical and chemical properties, comparing them to the five substances and which one matches. The chemical reactions with water, universal indicator, vinegar and Iodine solution are then analyzed and matched with each other to determine the mystery powder.
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).
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).
Aluminum is the most abundant metallic constituent in the crust of the earth; only the nonmetals oxygen and silicon are more abundant. Aluminum is never found as a free metal; commonly as aluminum silicate or as a silicate of aluminum mixed with other metals such as sodium, potassium, iron, calcium, and magnesium. These silicates are not useful ores, for it is chemically difficult, and therefore an expensive process, to extract aluminum from them. bauxite an impure h...
CaCl2 + H2O + CO2
Investigation of the heat energy produced by combustion of various alcohols. Aim: ---- To investigate how different alcohols produce different amounts of heat energy through combustion. I will be heating water using different alcohols as fuels and measuring the amount of fuel consumed.
heat will stay in the cup and can only escape by rising to the surface
Stated by The Columbia Encyclopedia, 6th Ed. It is said that “Charcoal is a substance obtained by partial burning or carbonization (destructive distillation) of organic material, a charcoal is largely pure carbon.” In addition, The Columbia Encyclopedia said that the entry of air during the carbonization process is controlled so that the organic material does not turn to ash, as in a conventional fire, but decomposes to form charcoal.
· When I have collected my results I will place them in a table like
In order to full under stand geothermal heating and cooling you first need to understand what geothermal energy is. Geothermal energy is a form of energy conversion that is provided by nature and that can be used by humans to cook, bath, heating and generate electric power. The energy is created by capturing and harnessing the heat energy. This heat is formed underground and is created by the radioactive decay of certain elements such as potassium, thorium, and uranium in Earth. One way to produce energy from geothermal heat is to use the heat to create steam to drive turbines that spin an electric generator, this method and others like it can create about 1,400,000 terawatt-years roughly three times the world’s annual consumption(Lund 2014).
Softening Hard Water With Sodium Carbonate Prediction ---------- In a preliminary experiment, we discovered that adding 1g. Na2CO3 to hard water softened it slightly. We tested both tap water and distilled water with the sodium stearate and discovered that tap water was far harder than distilled water, we then tested tap water that 1g of Na2CO3 had been applied to. This solution was softer than the original tap water.
Based on your experiments what is the formula of the colorless gas that is released when heating the malachite?
An Investigation into the Decomposition of Hydrogen Peroxide Aim: To investigate the rate of decomposition of H2O2 with different amounts of catalyst (MnO2). Hypothesis: When H2O2 and a catalyst are mixed together, the catalyst would break down H2O2 into water and oxygen. This will result in bubbles being produced. With the data of these oxygen bubbles, the rate at which H2O2 decomposed could be found out. 2H2O2 (l) à2H2O + O2 The controlwould be to maintain the same temperature (room temperature) and to use the same amount of hydrogen peroxide (10ml) in all the tubes.
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