Mercury molar mass

With these facts in mind, it seems reasonable to calculate the pore volume from the calibration curve that is accessible for a certain molar mass interval of the calibration polymer. A diagram of these differences in elution volume for constant M or AM intervals looks like a pore size distribution, but it is not [see the excellent review of Hagel et al. (5)]. Absolute measurements of pore volume (e.g., by mercury porosimetry) show that there is a difference on principle. Contrary to the absolute pore size distribution, the distribution calcu-... 

C05-0021.A 2.96-g sample of a compound of mercury and chlorine is vaporized in a 1.000-L bulb at 307 °C, and the final pressure is found to be 394 torr. What are the molar mass and chemical formula of the compound ... 

Matter occupies space, and matter is made up of atoms, so atoms occupy space. It is extremely difficult to compress a solid such as copper or a liquid such as mercury, because the electron cloud of each atom occupies some volume that no other atom is able to penetrate because of electron-electron repulsion. Example shows how to estimate the volume of an atom from the density of a sample, the molar mass of the substance, and Avogadro s number. 

This short overview illustrates the large complexity of the SEC processes and explains the absence of a quantitative theory, which would a priori express dependence between pore size distribution of the column packing—determined for example by mercury porosimetry—and distribution constant K in Equation 16.4. Therefore SEC is not an absolute method. The SEC columns must be either calibrated or the molar mass of polymer species in the column effluent continuously monitored (Section 16.9.1). 

Apparatus for cryoscopic determination of molar mass. The cryoscopic mercury thermometer can be replaced by a resistance thermometer or a calibrated thermistor. 

Ibf) force to accelerate l(lbm) by 32.1740 (ft) s" atm = standard atmospheric pressure = 101 325 Pa (psia) E pounds force per square inch absolute pressure torr = pressure exerted by 1 mm mercury at 273.15 K (0°C) and standard gravity (cal) = thermochemical calorie (Btu) s international steam table British thermal unit (lb mole) s mass in pounds mass with numerical value equal to the molar mass (R) - absolute temperature in Rankines... 

First calculate the molar enthalpy of fusion and molar enthalpy of vaporization, which have units of J/mol. Use the molar mass of mercury to convert from J/g to J/mol. 

Mercury(II) chloride (HgCl2) freezes at 276.1°C and has a freezing-point depression constant Xf of 34.3 K kg moU. When 1.36 g of solid mercury(I) chloride (empirical formula HgCl) is dissolved in 100 g of HgCl2, the freezing point is reduced by 0.99°C. Calculate the molar mass of the dissolved solute species and give its molecular formula. 

Plan This is a limiting-reactant problem because the amounts of two reactants are given. After balancing the equation, we must determine the limiting reactant. The molarity (0.010 M) and volume (0.050 L) of the mercury(II) nitrate solution tell us the moles of one reactant, and the molarity (0.10 M) and volume (0.020 L) of the sodium sulfide solution tell us the moles of the other. Then, as in Sample Problem 3.10, we use the molar ratio to find the moles of HgS that form from each reactant, assuming the other reactant is present in excess. The limiting reactant is the one that forms fewer moles of HgS, which we convert to mass using the HgS molar mass. The roadmap shows the process. 

Mercury and chlorine, for example, combine to form a compound that is 73.9% mercury and 26.1% chlorine by mass. Thus, if we had a 100.0-g sample of the compound, it would contain 73.9 g of mercury and 26.1 g of chlorine. (Samples of any size can be used in problems of this type, but we will generally use 100.0 g to simplify the calculation of mass from percentage.) Using atomic weights to get molar masses, we can calculate the number of moles of each element in the sample ... 

Check Water has a density of 1.00 g/cm, which can be converted to 1000kg/m Our estimate that the density of mercury is 14 times higher than water seems reasonable, given the fact that the molar mass of Hg is approximately 11 times larger than water. 

Determine the molar mass of each of the following compounds, all of which have been used as explosives (a) lead azide, PbN, (b) nitroglycerin, C3H5N5O9, (c) mercury fulminate, Hg(ONC)2... 

Looking at these three compounds, we see that nitroglycerin has the smallest molar mass even though it clearly contains the most atoms per molecule. Does this make sense The key factor is that both lead azide and mercury fulminate contain elements with large molar masses, so it is not surprising that nitroglycerin is the least massive of these three molecules. 

The mass cf cne mole of a pure substance is called the molar mass of that substance. Molar mass is usually written in units of g/mol. The molar mass of an element is numerically equal to the atomic mass of the element in unified atomic mass units (which can be found in the periodic table). For example, the molar mass of Uthium, Li, is 6.94 g/mol, while the molar mass of mercury, Hg, is 200.59 g/mol (rounding each value to two decimal places). The molar mass of an element contains one mole of atoms. For example, 4.00 g of helium, 6.94 g of Uthium, and 200.59 g of mercury all contain a mole of atoms. Figure 3.6 shows molar masses of three common elements. 

The molar mass of mercury Hg is M = 200.59 g/mol. In the calculation, equiUbrium with a free, plane surface of mercury is assumed, and mercury vapour Hg(g) is assumed to be an ideal gas. 

The molar mass of radon gas was first estimated by comparing its diffusion rate with that of mercury vapor, Hg(g). What is the molar mass of radon if mercury vapor diffuses 1.082 times as fast as radon gas Assume that Graham s law holds for diffusion. 

Three ways of quantitatively expressing the concentration of a solution will be presented here Mass/mass percent, %(m/m), mass/volume percent, %(m/v), and molarity, M. A fourth, molality, will appear later in this chapter. You should know an interesting fact about concentrations. No matter what size sample of a solution you have, be it a teaspoonful or a bucketful, the concentration is the same for both. This is because concentrations are stated in terms of the amount of solute in a fixed amount of solvent 100 g, 100 mL, or 1.00 L. It s like density. The density of mercury is 13.6 g/mL. If I have 100 mL or three drops of mercury, the density of mercury is still 13.6 g/mL. Neither density nor concentration depends on the size of the sample. 

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