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Is the production of CO2 from limestone is economically viable?
Wiki User
∙ 13y ago
The production of CO2 from limestone, known as calcination, is not a direct way to produce CO2 as it releases it as a byproduct. Economically, this process can be viable in industries that can capture and utilize the released CO2, such as in the production of cement or in carbon capture and storage technologies.
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Which rock removes CO2 from the atmosphere?
Limestone rocks remove CO2 from the atmosphere through a process called weathering. When exposed to rainwater and carbon dioxide, limestone undergoes chemical reactions that convert CO2 into calcium bicarbonate, which eventually ends up in the ocean through rivers, effectively sequestering the carbon.
What is the symbol equation for heating limestone?
The symbol equation for heating limestone (calcium carbonate) is: CaCO3(s) → CaO(s) + CO2(g) where limestone decomposes into calcium oxide and carbon dioxide upon heating.
What is the formula of creating quicklime from limestone?
Quicklime is created from limestone through a process called calcination. The chemical equation for this process is: CaCO3 (limestone) -> CaO (quicklime) + CO2 (carbon dioxide). It involves heating limestone to high temperatures, around 900-1000°C, to drive off the carbon dioxide and produce quicklime.
What happens if you heat limestone?
Limestone is calcium carbonate (CaCO3) which when heated to above 840°C decomposes into calcium oxide (CaO) while releasing carbon dioxide (CO2) according to the equation: CaCO3 → CaO + CO2
What element do soda limestone and sand all contain?
Soda limestone and sand all contain the element "silicon."
What will happen when limestone is heated at a high temperature?
It will decompose according to: CaCO3(s) --> CaO(s) + CO2
Which rock removes CO2 from the atmosphere?
Limestone rocks remove CO2 from the atmosphere through a process called weathering. When exposed to rainwater and carbon dioxide, limestone undergoes chemical reactions that convert CO2 into calcium bicarbonate, which eventually ends up in the ocean through rivers, effectively sequestering the carbon.
The gas given off when limestone is heated?
Carbon Dioxide (CO2)
What is the name and formula of the gas that is also produced when limestone is heated?
Carbon dioxide (CO2). The reaction is CaCO3--->CaO + CO2.
What is the symbol equation for heating limestone?
The symbol equation for heating limestone (calcium carbonate) is: CaCO3(s) → CaO(s) + CO2(g) where limestone decomposes into calcium oxide and carbon dioxide upon heating.
What is the balanced chemical equation for the decomposition of limestone to form calcium oxide and carbon dioxide?
The balanced chemical equation for the decomposition of limestone (CaCO3) to form calcium oxide (CaO) and carbon dioxide (CO2) is: CaCO3 -> CaO + CO2
What is the formula of creating quicklime from limestone?
Quicklime is created from limestone through a process called calcination. The chemical equation for this process is: CaCO3 (limestone) -> CaO (quicklime) + CO2 (carbon dioxide). It involves heating limestone to high temperatures, around 900-1000°C, to drive off the carbon dioxide and produce quicklime.
What happens if you heat limestone?
Limestone is calcium carbonate (CaCO3) which when heated to above 840°C decomposes into calcium oxide (CaO) while releasing carbon dioxide (CO2) according to the equation: CaCO3 → CaO + CO2
What element do soda limestone and sand all contain?
Soda limestone and sand all contain the element "silicon."
CO2 production from 1 gallon gasolene?
yes there is CO2 that comes out of gasoline
How are limestone caves different to other caves?
Primarily in their mode of formation: dissolution of limestone by water acidified by atmospheric CO2 (forming carbonic acid).
What mass of carbon dioxide would be produced when 2.00g of limestone is heated?
The chemical formula for limestone is CaCO3. When heated, limestone decomposes to produce calcium oxide (CaO) and carbon dioxide (CO2). The molar mass of CaCO3 is 100.09 g/mol. To calculate the mass of CO2 produced, you would first calculate the moles of CaCO3 in 2.00g, then use the stoichiometry from the balanced chemical equation to determine the moles and then mass of CO2 produced.
