Limestone loses mass when heated because of a chemical change: the gas carbon dioxide (CO2) is released by a chemical process when the rock is heated. The heat turns some of the calcium carbonate of the limestone into calcium oxide (quicklime) and carbon dioxide.
To calculate the mass of calcium oxide produced from 4.7 kg of calcium carbonate, you need to know the molar mass of calcium carbonate (CaCO3) and calcium oxide (CaO), as well as the stoichiometry of the reaction between these two compounds. This information will allow you to determine the theoretical yield of calcium oxide that can be obtained from the given mass of calcium carbonate.
The molar mass of calcium carbonate (CaCO3) is 100.09 g/mol. To find the mass of 0.250 mol of calcium carbonate, you would multiply the number of moles by the molar mass: 0.250 mol x 100.09 g/mol = 25.02 grams of calcium carbonate.
This question is solved with the help of mole concept . 1 mole of anhydrous calcium carbonate weighs 40+12+48=100 gm . 1.25 mole of similar anhydrous calcium carbonate will be 100* 1.25 = 125 gm
The molar ratio between calcium carbonate and calcium oxide is 1:1. So, 25 moles of calcium carbonate will produce 25 moles of calcium oxide. The molar mass of calcium oxide is 56.08 g/mol, so the mass of calcium oxide produced will be 25 moles * 56.08 g/mol = 1402 g.
To find the mass of calcium carbonate in a Tums tablet, you can weigh the tablet before and after a reaction that specifically targets the calcium carbonate. For example, if you react the tablet with hydrochloric acid to produce carbon dioxide gas, you can measure the mass lost due to the evolution of CO2 to calculate the mass of calcium carbonate present.
Many antacids and calcium supplements contain calcium carbonate.
Calcium carbonate (CaCO3) consists of one calcium ion (Ca2+) and one carbonate ion (CO3^2-). Therefore, the percentage of calcium ions in calcium carbonate is calculated as: (Atomic mass of calcium / Molecular mass of calcium carbonate) x 100 = (40.08 / 100.09) x 100 = 40.02% Therefore, calcium ions make up approximately 40.02% of the total mass of calcium carbonate.
The molar mass of calcium carbonate (CaCO3) is 100.09 g/mol. To calculate the percent mass of calcium, you need to divide the molar mass of calcium (40.08 g/mol) by the molar mass of calcium carbonate. This gives you a result of 0.4006, meaning that calcium constitutes approximately 40.06% of the mass of calcium carbonate.
The molar mass of calcium carbonate (CaCO3) is 100.09 g/mol. Therefore, the mass of 0.5 moles of calcium carbonate would be 0.5 mol x 100.09 g/mol = 50.045 grams.
CaCO3(s) ==heat==> CaO(s)+CO2(g) The correct chemical expression you need is NOT 'heated' , but 'Thermal Decomposition'. Calcium carbonate when heated to about 900 oC ( red glowing heat) will undergo thermal decomposition , to form calcium oxide((quick)lime) and carbon dioxide. Visually, you don't see anything. Calcium carbonate is white in coliur as is Calcium Oxide. You do not see carbon dioxide being given off. The only way to check is by weighing the mass of calcium carbonate. Heat it. Re-weigh when cool. It shoulk be of less weight. The difference being the mass of CO2 liberated, which you cannot weigh.
For a partly ionically bonded compound such as calcium carbonate, the gram formula mass is substituted for a mole, which technically exists only for purely covalently bonded compounds. The gram formula mass for calcium carbonate is 100.09. Therefore, 200 grams constitutes 200/100.09 or 2.00 gram formula masses of calcium carbonate, to the justified number of significant digits.
To calculate the mass of calcium oxide produced from 4.7 kg of calcium carbonate, you need to know the molar mass of calcium carbonate (CaCO3) and calcium oxide (CaO), as well as the stoichiometry of the reaction between these two compounds. This information will allow you to determine the theoretical yield of calcium oxide that can be obtained from the given mass of calcium carbonate.
The mass of sodium bicarbonate (NaHCO3) is 84 grams/mol, while the mass of calcium carbonate (CaCO3) is 100 grams/mol. Therefore, calcium carbonate has a higher molecular mass compared to sodium bicarbonate.
2,8 moles of calcium carbonate have 240,208 g.
The molar mass of calcium carbonate (CaCO3) is 100.09 g/mol. To find the mass of 0.250 mol of calcium carbonate, you would multiply the number of moles by the molar mass: 0.250 mol x 100.09 g/mol = 25.02 grams of calcium carbonate.
When limestone is heated, it undergoes a chemical reaction that releases carbon dioxide gas, leaving behind calcium oxide. As a result, the mass of the limestone would be greater than the mass of the calcium oxide produced, due to the loss of carbon dioxide during the reaction.
This question is solved with the help of mole concept . 1 mole of anhydrous calcium carbonate weighs 40+12+48=100 gm . 1.25 mole of similar anhydrous calcium carbonate will be 100* 1.25 = 125 gm