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# what is the temperature required for the decomposition of caco3 in degree celsius

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### Mohammed

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## physical chemistry

Thermal decomposition of calcium carbonate. In general, we heat \$\ce{CaCO3}\$ to temperature of approximately 825°C it decomposes into calcium oxide and liberates carbon dioxide gas:* \$\$\ce{CaCO3} \

## Thermal decomposition of calcium carbonate

Asked 8 years, 6 months ago

Modified 3 years ago

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Thermal decomposition of calcium carbonate.

In general, we heat CaCO 3 CaCOX3

to temperature of approximately 825°C it decomposes into calcium oxide and liberates carbon dioxide gas:*

CaCO 3 ⟶ 825 ∘ C CaO+CO 2

CaCOX3⟶825 ∘CCaO+COX2

Is it possible to heat the calcium carbonate at temperatures below 825 degrees Celsius.

physical-chemistry thermodynamics Share

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edited Feb 10, 2014 at 15:15

asked Feb 10, 2014 at 14:19

Do you mean "Is it possible to achieve the same effect heating the calcium carbonate at temperatures below 825 degrees Celsius?" –

G M

Feb 10, 2014 at 14:54

Yes, complete calcite at temperatures below 825 degrees Celsius. –

marco2008

Feb 10, 2014 at 15:58

2

Pump a hard vacuum and calcium carbonate will calcine at a lower temperature. 825°C is about one atmosphere of carbon dioxide at equilibrium. Thermodynamics proposes, kinetics disposes - finely ground goes faster than bulk.

answered Feb 10, 2014 at 17:33

In the US we activate molecular sieves in a vacuum oven around 150-200 C. In Canada, they use porcelain bowl and a Meeker burner underneath. If nanostructure is important, go cooler. –

Uncle Al

Feb 10, 2014 at 23:10

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स्रोत : chemistry.stackexchange.com

## Does anybody know how to reduce decomposition temperature of Calcium Carbonate?

Question

Parvin Golbayani Lhoist NA

## Does anybody know how to reduce decomposition temperature of Calcium Carbonate?

I know that Calcium carbonate decomposes into calcium oxide and carbon dioxide when heated above 840 °C. I am wondering if there is any way to reduce that decomposition temperature chemically? by adding some chemicals that could act as a catalyzed. Or other exciting ways...Any idea or comment?

Thanks. Calcium Oxide Calcium Carbonate Carbon Dioxide Decomposition

11th Jan, 2021 Frank Veroustraete REDSTAR CV&M

- Yes Henrik, a pressure reduction would be pretty beneficial to increase the overall efficiency of the FBC process. The gain in efficiency should be evaluated.

- And Yes Ammasi, there are a lot of techniques which can be tested with an FBC process approach, including the ones you cited.

- Hi Robin. I am not sure whether CaCl2 is useful when you want to produce cement. Is CaO not the product you want, to produce cement? Calcium chloride is commonly encountered as a hydrated solid with generic formula CaCl2(H2O), where = 0, 1, 2, 4, and 6. These compounds are mainly used for deicing and dust control. Because the anhydrous salt is hygroscopic, it is used as a desiccant.

Cheers and a happy New 2021!

Frank Cite 1 Recommendation

29th Sep, 2014 Frank Veroustraete REDSTAR CV&M Hi Parvin,

Calcination reactions usually take place at or above the thermal decomposition temperature (for decomposition and volatilization reactions) or the transition temperature (for phase transitions). This temperature is usually defined as the temperature at which the standard Gibbs free energy for a particular calcination reaction is equal to zero. For example, in limestone calcination, a decomposition process, the chemical reaction is

CaCO3 → CaO + CO2(g)

The standard Gibbs free energy of reaction is approximated as ΔG°r = 177,100 − 158 T (J/mol).[3] The standard free energy of reaction is zero in this case when the temperature, T, is equal to 1121 K, or 848 °C.

Examples of chemical decomposition reactions common in calcination processes, and their respective thermal decomposition temperatures include:

CaCO3 → CaO + CO2; 848 °C

Calcination of limestone using charcoal fires to produce quicklime has been practiced since antiquity by cultures all over the world. The temperature at which limestone yields calcium oxide is usually given as 825 °C, but stating an absolute threshold is misleading. Calcium carbonate exists in equilibrium with calcium oxide and carbon dioxide at any temperature. At each temperature there is a partial pressure of carbon dioxide that is in equilibrium with calcium carbonate. At room temperature the equilibrium overwhelmingly favors calcium carbonate, because the equilibrium CO2 pressure is only a tiny fraction of the partial CO2 pressure in air, which is about 0.035 kPa.

At temperatures above 550 °C the equilibrium CO2 pressure begins to exceed the CO2 pressure in air. So above 550 °C, calcium carbonate begins to outgas CO2 into air. However, in a charcoal fired kiln, the concentration of CO2 will be much higher than it is in air. Indeed if all the oxygen in the kiln is consumed in the fire, then the partial pressure of CO2 in the kiln can be as high as 20 kPa.[36]

The table shows that this equilibrium pressure is not achieved until the temperature is nearly 800 °C. For the outgassing of CO2 from calcium carbonate to happen at an economically useful rate, the equilibrium pressure must significantly exceed the ambient pressure of CO2. And for it to happen rapidly, the equilibrium pressure must exceed total atmospheric pressure of 101 kPa, which happens at 898 °C.

Equilibrium pressure of CO2 over CaCO3 (P) vs. temperature (T).[37]

P (kPa) 0.055 0.13 0.31 1.80 5.9 9.3 14 24 34 51 72 80 91 101 179 901 3961

T (°C) 550 587 605 680 727 748 777 800 830 852 871 881 891 898 937 1082 1241

But, three Au/TiO2 catalysts, with the same Au loading and with different particle sizes, were prepared by the deposition–precipitation method followed by calcination at three different temperatures, 473, 573, and 873 K. The mean diameters of Au particles were 2.4, 2.5, and 10.6 nm, respectively. On all the samples the CO adsorption and different CO–O2 interactions were examined by FTIR at 90 K and at room temperature. The higher catalytic activity on CO oxidation found for the samples calcined at 473 and 573 K is related to the higher concentration of step sites over the Au surfaces and to a higher concentration of step sites at the borderline with the support. At 90 K, CO and molecular oxygen are competitively adsorbed on step sites. By CO pre-adsorption on hydrated catalysts, the reaction with O2 gives CO2 already at 90 K, while by oxygen pre-adsorption the reaction is completely inhibited, unless moisture is present in the gas phase.

Hence Parvin, the Au/TiO2 catalyst seems to have the desired effect on the reduction of calcination temperature. Check it out and save energy!

Cheers, Frank Cite

स्रोत : www.researchgate.net

## Decomposition temperature of CaCO(3)(s) is approximately 900^(@)C. Which of the following decompose below 900^(@)C?

More is covalent character, lesser is the thermal stability

Home > English > Class 12 > Chemistry > Chapter > Test Papers >

Decomposition temperature of C...

Decomposition temperature of

CaC O 3 (s) CaCO3(s) is approximately 900 ∘ C 900∘C

. Which of the following decompose below

900 ∘ C 900∘C ?

Updated On: 27-06-2022

Get Answer to any question, just click a photo and upload the photo and get the answer completely free,

Text Solution A BeC O 3 ,MgC O 3 BeCO3,MgCO3 B SrC O 3 ,BaC O 3 SrCO3,BaCO3 C BeC O 3 ,BaC O 3 BeCO3,BaCO3 D MgC O 3 ,SrC O 3 MgCO3,SrCO3 Answer

Solution

More is covalent character, lesser is the thermal stability

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646686576 0 7.6 K 2:58

Decomposition temperature of

CaC O 3 (s) CaCO3(s) is approximately 900 ∘ C 900∘C

. Which of the following decompose below

900 ∘ C 900∘C ? 643124294 13 1.9 K

निम्न अभिक्रिया के लिए

atm

900 ∘ C 900∘C पर K p =1.04 Kp=1.04

CaC O 3 (s)→CaO(s)+C O 2 (g)

CaCO3(s)→CaO(s)+CO2(g)

. निम्न ताप पर 58.4gC

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Mohammed 4 month ago

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