Calculating from moles

Calculated from mole fractions and molecular weights of SRC-II-Acid (M — 210) and Et3N (M = 101) assuming no complex formation. 

Using this concept, Burdett developed a method in 1955 to obtain the concentrations in mono-, di- and polynuclear aromatics in gas oils from the absorbances measured at 197, 220 and 260 nm, with the condition that sulfur content be less than 1%. Knowledge of the average molecular weight enables the calculation of weight per cent from mole per cent. As with all methods based on statistical sampling from a population, this method is applicable only in the region used in the study extrapolation is not advised and usually leads to erroneous results. 

A7 Ethane/methane selectivity calculated from grand canonical Monte Carlo simulations of mixtures in slit IS at a temperature of 296 K. The selectivity is defined as the ratio of the mole fractions in the pore to the ratio of mole fractions in the bulk. H is the slit width defined in terms of the methane collision diameter (Tch,- (Figure awn from Crackncll R F, D Nicholson and N Quirke 1994. A Grand Canonical Monte Carlo Study ofLennard-s Mixtures in Slit Pores 2 Mixtures of Two-Centre Ethane with Methane. Molecular Simulation 13 161-175.)... 

If the number of equivalents per mole is known, the molecular weight is calculated from the equivalent weight by multiplying the latter by the number of equivalents per mole. 

If the initiation reaction is much faster than the propagation reaction, then all chains start to grow at the same time. Because there is no inherent termination step, the statistical distribution of chain lengths is very narrow. The average molecular weight is calculated from the mole ratio of monomer-to-initiator sites. Chain termination is usually accompHshed by adding proton donors, eg, water or alcohols, or electrophiles such as carbon dioxide. 

The interfacial mole fractions yj and Xj can be determined by solving Eq. (5-252) simultaneously with the equilibrium relation = F(x,) to obtain y and Xj. The rate of transfer may then be calculated from... 

Transfer units may he calculated from Eq. 14-25, replacing mole fractions with ppm concentrations, and since the operating and eqnihhrinm hnes are straight,... 

If the total pressure of a mixture is known, the partial pressure of each component can be calculated from the mole fraction. The total number ol moles in the mixture is the sum of the individual component moles. 

Rate constants (fifth column) usually correspond to one of the temperatures reported in the original papers and may be either experimentally determined values or those calculated from the activation parameters. In the preparation of the present review, the author has normalized a number of rate constants at arbitrary temperatures to permit direct comparisons with other data these normalized values and temperatures are tabulated (in italics) with the hope that they will offer additional useful information. The rate constants are usually expressed in liter x mole x sec when the values are followed by the symbol (A i) the units are sec. and dH are in kcal/mole JS is in eu. 

The label on a bottle of concentrated hydrochloric acid. The label gives the mass percent of HCI in the solution (known as the assay] and the density (or specific gravity) of the solution. The molality, molarity, and mole fraction of HCI in the solution can be calculated from this information. 

It is possible (but not easy) to calculate from K the extent to which N02 is converted to N204 when the system is compressed. The results of such calculations are given in Table 12.6. As the pressure is increased from 1.0 to 10.0 atm, more and more of the N02 is converted to N204. Notice that the total number of moles of gas decreases steadily as a result of this conversion. 

Consider the substance hydrogen chloride. This compound has the molecular formula HQ. A chemist working with hydrogen chloride, HQ, must often know the weight of a mole of molecules (the molecular weight). This weight is readily calculated from the atomic weights of the two kinds of atoms, H and Cl ... 

Fig. 10. The mole fraction of carbon dioxide in saturated solutions in air at — 110°C (above the lower critical end point). The full line is the experimental curve of Webster and the dashed curves are 1, an ideal gas mixture 2, an ideal gas mixture with Poynting s correction and 3, the solubility calculated from Eq. 8 and the principle of corresponding states.

The relative neutralizing capacity (RNC) of amines can be calculated from the reaction mole ratios thus, from the reaction of ammonia with carbonic acid, shown here, the RNC is 17/44 = 0.386 ppm neutralizing amine required per ppm C02 ... 

Fig. 17. Influence of bubble size on NAj as affected by interaction between bubbles (as a function of a in subreactors and for constant gas holdup), chemical reaction rates, and contact times. NAJ was calculated from Eq. (176) with c, = 1.46 x 10-7 gr-mole/cm3 D= 2.3 x 10"5 cm2/sec G> =0.064 d = 0.1 cm 0 = 2.85 sec [after Gal-Or and Hoel-scher (G5)].

An alternate way of calculating this entropy discrepancy is to attribute it to the mixing of two forms of CO that differ by having C and O reversed. The entropy of mixing 1/2 mole of each form is So and can be calculated from... 

The quantity Q can be calculated from a knowledge of the chemical reaction. If n moles of electrons are transferred from cathode to anode during the chemical reaction11 and F is the quantity of electrical change carried by a mole of electrons, then... 

STRATEGY To use Eq. 14, we need the total pressure (given) and the mole fraction of each component. The first step is to calculate the amount (in moles) of each gas present and the total amount (in moles). Then calculate the mole fractions from Eq. 12. To obtain the partial pressures of the gases, multiply the total pressure by the mole fractions of the gases in the mixture (Eq. 14). 

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