Plotted curves

These high values of 6c/6 , are not permissible. Plot curves for r/T < 1 also for settings at higher currents. 

A plotted curve as shown on Figure 3-59 [33] show s that at point A a rise of 20°F on the temperature rise curve corresponds to a flow of 47 GPM minimum safe for the pump handling 220°F, with NPSH of 18.8 feet. 

Plot curve of 1/ (yj - Xj) versus xj see Figure 8-38, graphical integration by Simpson s rule. 

Since the designer will be expected to plot curves to suit requirements, some examples will be cited that can serve as a guide for potential needs (Fig. 2-42). 

As mentioned, the data obtained by this method are expressed as cumulative size distribution curves. Since the computations assume Stokes law for spherical particles, the plotted curves give the distribution of spherical particles which would behave like the actual sample with respect to this experiment. For this reason, the sizes on the distribution curves should be labelled Stokes Equivalent Diameter . Because of the underlying assumptions and the above interpretation of the results, it is clear that the repeatability of this method has more meaning than accuracy of comparison with results of other methods... 

In each case, we draw the tangent line to the plotted curve. 

Effect of bandpass and choice of wavelength on a Beer s law plot. Curve A represents a calibration curve using a narrow bandpass monochromator at k. Curve B represents a calibration curve using a wide bandpass filter at X or a narrow bandpass monochromator at. ... 

The mathematical model may not closely fit the data. For example. Figure 1 shows calibration data for the determination of iron in water by atomic absorption spectrometry (AAS). At low concentrations the curve is first- order, at high concentrations it is approximately second- order. Neither model adequately fits the whole range. Figure 2 shows the effects of blindly fitting inappropriate mathematical models to such data. In this case, a manually plotted curve would be better than either a first- or second-order model. 

The relationship between /(O D) 05 and [H02] + [R02] is better illustrated in Fig. 6.32, which shows plots of both the square root and first power of /(O D) against the measured peroxy radical concentrations the square root plot is linear, while the first-order plot curves significantly. 

Since porosity-radius curves have been obtained, it is possible to plot curves of Dm against radius for the reacted rods. To correct to the temperature of reaction, it is assumed that Dm is proportional to 128). 

Plotted curves illustrating this relation, Fig. 5, resemble very much the curves of Fig. 3. Consequently, one cannot infer from a measured intensity or energy saturation curve reliable values of molecular data without additional information, as for instance an independent measurement of ksr Another possibility is a measurement of the temporal characteristics of the bleaching as demonstrated in an experiment by Hercher et al. 14>. These authors bleached a thoroughly degassed solution of metal-free phthalocyanine in 1-chloronaphthalene by a ruby laser pulse (694.3 nm) of about 59 nsec pulse width. At the same time they measured the absorption at 632.8 nm using a He-Ne-laser, and the result of this measurement is shown in Fig. 6. It clearly demonstrates that the sample was almost completely bleached even before the laser pulse reached its maximum intensity, and that almost all of the molecules were stored in the triplet state because the transmission did not decrease with the fall of the laser intensity for at least 100 nsec. A small residual absorption indicates triplet-triplet absorption. 

Calibration is carried out using the external standard method. The calibration curve was linear for each of nine BAs in the range of 5-100 nmol/ml. The resulting concentrations were extrapolated by the plotted curve. 

As a second trial, put r,/r2 = 2.3. This gives (ARcomp), - 1.5 and (YfcompWx - 23°. Marking off 23° to the left of the vertical -180° axis gives point A on the uncompensated plot (curve (i)—Fig. 7.64). The frequency at this point is [Pg.643]

Dichloromethane, CH2C12, is an organic solvent used for removing caffeine from coffee beans. The following table gives the vapor pressure of dichloromethane at various temperatures. Fill in the rest of the table, and use the data to plot curves of Pv ... 

Figure 7.11 shows modified Crawford-Wilke [11] correlation plot curves. Note that the y-axis is a type of Reynolds number, as discussed in Chap. 6. This y-axis number is similar to the Reynolds number, having density (Dc), viscosity (Uc), and velocity (Vc and Vd). If you review Chap. 6 and the Reynolds number, the same dimensional analysis is seen in the order given in Fig. 7.11 on the y-axis. The x-axis relates to viscosity (Uc), surface tension (0 ), density (Dc), and packing size factor (FJ. Originally the square root of the x-ordinate was used in the Crawford-Wilke correlation plotted against such a Reynolds number. Also, only one curve was made in this original work, the top curve labeled Crawford-Wilke in Fig. 7.11. This top curve represents the point at which the continuous phase is saturated with solute, in equilibrium condition. Eckert [9] reported that when Vc is increased, beginning at Vc = 0, the system floods before Vc reaches this saturation Crawford-Wilke curve.

Figure 2 Plots of the logarithm of electron transfer rate vs. the negative of the free energy of the reaction for three ET models and six rate measurements. The data are from Refs. 54, 55, 57, 59, 60 for a Zn-substituted Candida krusei cytochrome c that was also successively substituted at histidine 33 by three Ru(NH3)4L(His 33)3+ derivatives with L = NH3, pyridine, or isonicotinamide. The shortest direct distance between the porphyrin and imidazole carbon atoms was 13 A corresponding to the 10-A edge-to-edge D/A distance. Table 1 presents a summary of the parameters used in the three calculations plotted in this figure. For a (3 of 1.2 A-1, Eq. (5) yields HAB values ( 10 cm-1) of 80 cm-1,50 cm-1, and 75 cm-1, respectively, for Eq. (1), the semiclassical model [Eq. (4)], and the Miller-Closs model at the above D/A separation distance. The s values were calculated using Eq. (6) with the following parameters aD = 10 A, aA = 6 A, and r = 13 A. The kj and H°B parameters were varied independently to produce the plotted curves.

The fact that the analytical presentations of the pi-relationships encountered in engineering literature often take the shape of power products does not stem from certain laws inherent to dimensional analysis. It can be simply explained by the engineer s preference for depicting test results in double-logarithmic plots. Curve sections which can be approximated as straight lines are then analytically expressed as power products. Where this proves less than easy, the engineer will often be satisfied with the curves alone, cf. Fig 1. 

Full signs downflow, hollow signs upflow. Plotted curve Homogenization characteristics of Newtonian liquids, from [41]. 

Fig. 3.15. J-V characteristics of Schottky diodes with b- For a non-zero Schottky barrier curves B deviate from curves A as applied voltages increases. Curves B become straight lines at higher voltages where C is large. These straight lines correspond to Ohm s law as predicted by Eq. (3.49). The values of the parameters in these calculations are the same as given in Fig. 3.11 [44],...

Equation (3.2) expresses G as a function of volume and temperature. We wish it as a function of pressure and temperature, and it cannot conveniently be put in this form in an analytic way, on account of the difficulty of solving Van der Waals equation for the volume. It is an easy matter to compute a table of values, however. We plot curves, like Fig. XII-3, for pressure as a function of volume in Van der Waals equation, compute values of G from Eq. (3.2) for a number of values of the... 

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