The volume of carbon dioxide is 8,4 L at oC.
1.26
0.597
It is CaCO3.....it is the same as marbleFormula: CaCO3
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 .
CaCO3 (Calcium Carbonate)
CaCO3 --> CaO + CO2
Caco3% in marble grade lime stone
CaCO3
Calcium carbonate is not soluble in water.
CaCO3 + 2HCl -> CaCl2 + CO2 +H2O
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 !
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
15.2 g CaCO3 / 100.1 g CaCO3 x 22.4 L (STP)=3.40 L
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.
Normal pressure & above 840 degrees C.
It is CaCO3.....it is the same as marbleFormula: CaCO3
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 .
CaCO3 (Calcium Carbonate)
Molar mass CaCO3 = 100.087 g/mol Moles CaCO3 = 152 g / 100.087 = 1.52 the ratio between CaCO3 and CO2 is 1 : 1 so we get 1.52 moles of CO2 At STP p=1 ATM and T = 273 K V = nRT / p = 1.52 x 0.0821 x 273 /1 = 34.1L