Question

При растворении 360 г известняка в избытке раствора азотной кислоты выделилось 66,2 л (н.у.) оксида углерода (IV). Определите массовую долю карбоната кальция в данном образце известняка

Answer 1

Ответ:

вот держи удачи.

если помог можно лучший ответ?

Answer 2

Calculation of the Mass Fraction of Calcium Carbonate in Limestone

To determine the mass fraction of calcium carbonate in the given sample of limestone, we need to use the information provided about the reaction between calcium carbonate and nitric acid.

According to the given information, 360 g of limestone (calcium carbonate) was dissolved in an excess of nitric acid, resulting in the release of 66.2 L (at standard temperature and pressure) of carbon dioxide gas (CO2).

The balanced chemical equation for the reaction between calcium carbonate and nitric acid is as follows:

CaCO3 + 2HNO3 -> Ca(NO3)2 + CO2 + H2O

From the balanced equation, we can see that 1 mole of calcium carbonate (CaCO3) reacts to produce 1 mole of carbon dioxide (CO2). The molar mass of CO2 is 44 g/mol.

To calculate the mass fraction of calcium carbonate in the limestone, we can use the following formula:

Mass Fraction = (Mass of Calcium Carbonate / Total Mass of Limestone) * 100

To find the mass of calcium carbonate, we need to convert the volume of carbon dioxide gas (66.2 L) to moles using the ideal gas law.

First, we need to convert the volume of CO2 gas to moles at standard temperature and pressure (STP). The molar volume of an ideal gas at STP is 22.4 L/mol.

Moles of CO2 = Volume of CO2 gas / Molar volume at STP Moles of CO2 = 66.2 L / 22.4 L/mol

Now, we can calculate the moles of calcium carbonate using the stoichiometry of the balanced equation.

Moles of CaCO3 = Moles of CO2

Finally, we can calculate the mass of calcium carbonate using the molar mass of CaCO3, which is 100.09 g/mol.

Mass of CaCO3 = Moles of CaCO3 * Molar