Calcium carbonate molar mass

Self-Test L.2B Carbon dioxide can be removed from power plant exhaust gases by combining it with an aqueous slurry of calcium silicate 2 C02(g) + H,0(l) + CaSiOds) — Si02(s) + Ca(HC03)2(aq). What mass of CaSiO, (having molar mass 116.17 g-mol ) is needed to react completely with 0.300 kg of carbon dioxide ... 

The desired quantity is the volume of solution. The available data are the molarity of HCl in solution, the mass of chalk, and the molar mass of CaCOo. In addition, two relations are required. One identifies cnalk as calcium carbonate by stating that the mass of chalk equals the mass of CaC0 . Another gives the stoichiometry by saying that two times the number of moles of CaCO equals the number of moles of HCl. The diagram showing the solution in this case occupies several screens a separate screen is used to show each application of a relation. 

For example, consider calcium carbonate. This substance has a mass density Pcaco, equals 2.6 g/cc. Suppose, 35 mg is dissolved in a liter of water, find the corresponding molarity. 

CaC03] is an equivalent molar concentration expressed in terms of moles of CaC03. Thus, to get the equivalent calcium carbonate mass concentration, it must be multiplied by CaC03 = 100. Therefore,... 

If 3.45 L of carbon dioxide are formed at 700°C and 0.980 atm, what number of moles and what mass of calcium carbonate has decomposed The molar mass of CaC03 is 100.1 g. 

What volume of 0.250 M HC (aq) is required to just completely consume 8.50 g of calcium carbonate, CaC03 The molar mass of CaC03 is 100.1 g. The balanced equation is... 

The raw mix mineralogical composition is obtained from the average sample chemical analysis multiplying the present oxides (a L.o.I. free basis) by fhe molar mass/ mineral ratio. The calcium and magnesium released CO2 can be calculated multiplying their percentages by the ratio between the molar masses of carbon dioxide and fhe oxides themselves ... 

Calcium carbonate is an ionic compound composed of Ca and 3 ions. One mole of calcium carbonate contains 1 mol of Ca and 1 mol of 003 ions. We calculate the molar mass by summing the masses of the components. 

We want to determine the molar mass of calcium carbonate in units of g/mol. 

The molar mass (M) of a substance is the mass in granns of 1 mole of the substance. By definition, the mass of a mole of carbon-12 is exactly 12 g. Note that the molar mass of carbon is numerically equal to its atomic mass. Likewise, the atomic mass of calcium is 40.08 amu and its molar mass is 40.08 g, the atomic mass of sodium is 22.99 amu and its molar mass is 22.99 g, and so on. In general, an element s molar mass in grams is numerically equal to its atomic mass in atomic mass units. The molar mass (in grams) of any compound is numerically equal to its molecular or formula mass (in amu). The molar mass of watCT, for example, is 18.02 g, and the molar mass of sodium chloride (NaCl) is 58.44 g. 

Solid calcium carbonate, CaC03(s), reacts with HCl(aq) to form H2O, CaCl2(aq), and C02(g). If a 45.0 g sample of CaC03(s) is added to 1.25 L of HCl(aq) that is 25.7% HCl by mass d = 1.13 g/mL), what will be the molarity of HCl in the solution after the reaction is completed Assume that the solution volume remains constant. 

Here we will use a simplified example to illustrate some basic aspects of the mass transport process for carbonates that avoids most of the more complex relationships. In this example, the calcium and carbonate ion concentrations are set equal, and values of the activity coefficients, temperature, and pressure are held constant. The carbonate ion concentration is considered to be independent of the carbonic acid system. The resulting simple (and approximate) relation between the change in saturation state of a solution and volume of calcite that can be dissolved or precipitated (Vc) is given by equation 7.4, where v is the molar volume of calcite. 

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