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Formula of limestone?
It is CaCO3.....it is the same as marbleFormula: CaCO3
When calcium carbonate is heated strongly carbon dioxide gas is released CaCO3CaO CO2 what is the volume of CO2 measured stpis produced if 1 grams of caco3 is heated?
When 1 gram of calcium carbonate (CaCO3) is heated, it decomposes to produce calcium oxide (CaO) and carbon dioxide (CO2). The molar mass of CaCO3 is approximately 100 g/mol, so 1 gram corresponds to about 0.01 moles of CaCO3. According to the reaction, 1 mole of CaCO3 produces 1 mole of CO2; thus, 0.01 moles of CaCO3 will produce 0.01 moles of CO2. At standard temperature and pressure (STP), 1 mole of gas occupies 22.4 liters, so the volume of CO2 produced is approximately 0.01 moles × 22.4 L/mol = 0.224 liters, or 224 mL.
Is caco3 insoluble when react with water?
caco3 is solid form. its density is high so caco3 is not soluble in water. but co2 mix in water befuor the mix in caco3 . so caco3 is soluble after mixing the co2 .
What is the balanced equation for caCO3 2HCI?
CaCO3 + 2HCl --> CaCl2 + H2O + CO2
Whats the limestone heating reaction?
When limestone (calcium carbonate) is heated, it undergoes thermal decomposition to produce calcium oxide (quicklime) and carbon dioxide gas. The chemical equation for this reaction is: CaCO3 (s) → CaO (s) + CO2 (g).
What conditions of temperature and pressure would get the most decompomposition of CaCo3?
Calcium carbonate (CaCO3) decomposes into calcium oxide (CaO) and carbon dioxide (CO2) at high temperatures. To maximize decomposition, high temperatures above 800 degrees Celsius and low pressures are ideal. These conditions will promote the breakdown of CaCO3 into its components.
What is the volume of CaCO3 if you have a molarity of 75.5 and 15 g CaCO3 What is the answer and how did you get it?
Calcium carbonate is not soluble in water.
CaCO3 -- CO2 CaO how many liters of CO2 at 1.03 ATM and a temperature of 950 degrees celsius will be produced if there is 1.00 kg of CaCO3 and what are the calculations to solve it or formulas?
1. First of all there is a 1:1 molar ratio. 2. 1000g CaCO3 3. Mass divided Mol Wt = 10 mols (CaCO3 = 100 g/mol) 4. 10 mols CaCO3 produces 10 mols CO2 5. Ideal Gas Law is PV = nRT P = Pressure = 1.03 ATM V = Is what you are solving for n = mols of CO2 = 10 R = Gas Law Constant (look it up either on the web or books in the units you are working with - ATM, celsius, liters OR convert them into something you do have) 6. Plug in the numbers and solve for V in liters - You're Done !
What volume of a 0.10 mol dm-3 solution of HCl is required to react with 10.0 g of CaCO3?
2 HCl + CaCO3 = CaCl2 + CO2 + H2O Therefore it takes twice as many moles of HCl to react with CaCO3 Mol CaCO3 = mass / formulae weight = 10 / 40.08 + 14.01 + 3(16.00) = 10 / 102.09 = 0.0980 mol Mol HCl = 2 x 0.0980 = 0.1959 mol Volume HCl = mol / c = 0.1959 / 0.10 = 1.9591 L Volume required to react of HCl = 1.9591 L
When calcium carbonate is heated strongly carbon dioxide gas is released CaCO3CaO CO2 what is the volume of CO2 measured stpis produced if 15.2 grams of caco3 is heated?
The molar mass of CaCO3 is 100.09 g/mol, and the molar mass of CO2 is 44.01 g/mol. By using stoichiometry, you can calculate that 15.2 grams of CaCO3 would produce 6.51 grams of CO2. Using the ideal gas law, you can then convert the mass of CO2 to volume using its molar volume at STP (22.4 L/mol). The volume of CO2 produced would be around 3.32 liters.
what would be the volume of CO2 (at STP) produced from the complete reaction of 10 grams of CaCO2?
Assuming complete reaction, the molar mass of CaCO3 is approximately 100.09 g/mol. One mole of CaCO3 produces one mole of CO2. Therefore, 10 grams of CaCO3 will produce approximately 2.24 liters of CO2 at STP (22.4 L/mol).
Which of the following salts has the greatest solubility in water at 25 degrees Celsius?
The salt with the greatest solubility in water is sodium chloride (NaCl). Sodium chloride is highly soluble in water due to its strong ionic bonds that readily break apart in water molecules, allowing it to dissociate into Na+ and Cl- ions.
What is the grams of substance in 4.5 moles CaCO3?
Molar mass of CaCO3 = 66.1221g CaCO3/mole CaCO3. This means that 1 mole CaCO3 = 66.1221g CaCO3. To find the mass of 4.5 mole CaCO3, complete the following calculation: 4.5g CaCO3 X 1mol CaCO3/66.1221g CaCO3 = 0.068 mole CaCO3.
What mass of caco3 is required to react with 100 ml of 2 m hcl solution?
To find the mass of CaCO3 required to react with 100 mL of 2 M HCl, you need to first calculate the number of moles of HCl using its molarity and volume. Then, use the balanced chemical equation to determine the mole ratio between HCl and CaCO3, allowing you to calculate the mass of CaCO3 needed.
Formula of limestone?
It is CaCO3.....it is the same as marbleFormula: CaCO3
How many grams of calcium carbonate are needed to produce 71.0 L of carbon dioxide at STP?
Assuming complete reaction, the molar volume of gas at STP is 22.4 L. Therefore, 71.0 L of CO2 corresponds to 71.0/22.4 = 3.17 moles of CO2. From the balanced chemical equation for the reaction of calcium carbonate (CaCO3) -> CaO + CO2, 1 mole of CaCO3 produces 1 mole of CO2. So, 3.17 moles of CO2 requires 3.17 moles of CaCO3. The molar mass of CaCO3 is 100.1 g/mol, so 3.17 moles of CaCO3 would be 3.17 * 100.1 = 317.6 grams of CaCO3.
When calcium carbonate is heated strongly carbon dioxide gas is released CaCO3CaO CO2 what is the volume of CO2 measured stpis produced if 1 grams of caco3 is heated?
When 1 gram of calcium carbonate (CaCO3) is heated, it decomposes to produce calcium oxide (CaO) and carbon dioxide (CO2). The molar mass of CaCO3 is approximately 100 g/mol, so 1 gram corresponds to about 0.01 moles of CaCO3. According to the reaction, 1 mole of CaCO3 produces 1 mole of CO2; thus, 0.01 moles of CaCO3 will produce 0.01 moles of CO2. At standard temperature and pressure (STP), 1 mole of gas occupies 22.4 liters, so the volume of CO2 produced is approximately 0.01 moles × 22.4 L/mol = 0.224 liters, or 224 mL.
