Exercises solutions

An aqueous solution of potassium iodide, KI, is heated from 25°C to 85°C. During the time period while the solution is being heated, which of the following is true  

If you were trying to increase the amount of dissolved carbon dioxide gas, CO2(g), in water, which set of conditions would allow you the highest levels of dissolved C02  

Which of the following solutions has the lowest freezing point  

An aqueous solution of silver nitrate (AgN03, molar mass 169.9 g) is prepared by adding 200.0 g AgNOa to 1,000 g HzO. If Kf for H20 is 1.86°C m 1, the freezing point of the solution should be 

A solution of glucose (molecular weight 180.16) in water (molecular weight 18.01) is prepared. The mole fraction of glucose in the solution is 0.100. What is the molality of 

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We will specifically consider water relations, solute transport, photosynthesis, transpiration, respiration, and environmental interactions. A physiologist endeavors to understand such topics in physical and chemical terms accurate models can then be constructed and responses to the internal and the external environment can be predicted. Elementary chemistry, physics, and mathematics are used to develop concepts that are key to understanding biology—the intent is to provide a rigorous development, not a compendium of facts. References provide further details, although in some cases the enunciated principles carry the reader to the forefront of current research. Calculations are used to indicate the physiological consequences of the various equations, and problems at the end of chapters provide further such exercises. Solutions to all of the problems are provided, and the appendixes have a large list of values for constants and conversion factors at various temperatures. 

Preparing solutions - practical advice is given on p. 15. A solution is a homogeneous liquid, formed by the addition of solutes to a solvent. The behaviour of solutions is determined by the type of solutes involved and by their proportions, relative to the solvent. Many laboratory exercises involve calculation of concentrations, e.g. when preparing an experimental solution at a particular concentration, or when expressing data in terms of solute concentration. Make sure that you understand the basic principles set out in this chapter before you tackle such exercises. Solutes can affect the properties of solutions in several ways, as follows. 

What happens to the rate of liver glucose metaholism during moderate-intensity exercise SOLUTION... 

Figure 3.13 LOPA Exercise Solution for the initial design.

Start-up kit consists of laboratory materials, as well as other required materials for successfully performing the exercise, such as source codes, scripts, and binary files, collected as separate archive files (e.g. tar, zip, or 7z), usually one archive per exercise, and sometimes an additional one archive for a course. In addition to laboratory exercise materials, some authors give a larger number of various supporting materials that can help the students, and make the process of conducting the exercise more effective. The materials are classified in terms of their purpose (lab instructions, work materials for students, exercise solution, tutorial documents, and tutorial examples) and scope of use (exercise, course). 

The use of Henry s constant for a standard-state fugacity means that the standard-state fugacity for a noncondensable component depends not only on the temperature but also on the nature of the solvent. It is this feature of the unsymmetric convention which is its greatest disadvantage. As a result of this disadvantage special care must be exercised in the use of the unsymmetric convention for multicomponent solutions, as discussed in Chapter 4. 

Dissolve 36 g. of sodium hydroxide in 160 ml. of water contained in a 500 ml. conical flask, and chill the stirred solution to 0-5° in ice-water. Now add io-8 ml. (32-4 g.) of bromine slowly to the stirred solution exercise care in manipulating liquid bromine ) during this addition the temperature rises slightly, and it should again be reduced to 0-5°. Add a solution of 12 g. of acetamide in 20 ml. of water, in small portions, to the stirred hypobromite solution so that the temperature of the mixture does not exceed 20° the sodium acet-bromoamide is thus obtained in the alkaline solution. Now remove the flask from the ice-water, and set it aside at room temperature for 30 minutes. 

Extend the matrix triangularization procedure in Exercise 2-14 by the Gauss-Jordan procedure to obtain the fully diagonalized matrix solution set follows routinely. 

If we go back and calculate the slope and intercept for the data set in Exercise 3-2 without the constraint that the line must pass through the origin, we get the solution vector 0.95, 0.09 for a line parallel to the line in Exercise 3-3 and 2.0 units distant from it, as expected. 

Select several values for p of the data set in Exercise 3-1 and calculate xi — p) for each of them. Plot the curve of xi — p) as a function of the selected parameter p and locate the minimum visually. Compare with Solution 3-1. 

Part A. In Exercise 6-3 we found that the closed solutions for the integral Eq. (6-23)... 

How many iterations does it take to achieve self-consistency for the helium problem treated (partially) in Exercises 8-3 and 8-4 What is the % discrepancy between the calculated value of the first ionization potential and the experimental value of 0.904 hartiees when the solution has been brought to self-consistency ... 

Generalize the solution of Exercise 9-1 to the case of a many-electron wave function [Eq. (9-29)] yielding Pm permutations. 

If all the above methods fail, the solution should be left in an ice chest (or a refrigerator) for a prolonged period. The exercise of considerable patience is sometimes necessary so as to give the solution every opportunity to crystallise. 

Other sources of hazard arise from the handling of such chemicals as concentrated acids, alkalis, metallic sodium and bromine, and in working with such extremely poisonous substances as sodium and potassium cyanides. The special precautions to be observed will be indicated, where necessary, in the experiments in which the substances are employed, and will also be supplied by the demonstrator. The exercise of obvious precautions and cautious handling will in most cases reduce the danger to almost negligible proportions. Thus, if concentrated sulphuric acid should be accidentally spilled, it should be immediately washed with a liberal quantity of water or of a solution of a mild alkali. 

Great caro must be exercised in handling ethyl bromoacetate. Keep a 10 per cent, aqueous ammonia solution available to react with any bromoester which may be spilled. 

Recovery of the wopropyl alcohol. It is not usually economical to recover the isopropyl alcohol because of its lo v cost. However, if the alcohol is to be recovered, great care must be exercised particularly if it has been allowed to stand for several days peroxides are readily formed in the impure acetone - isopropyl alcohol mixtures. Test first for peroxides by adding 0-6 ml. of the isopropyl alcohol to 1 ml. of 10 per cent, potassium iodide solution acidified with 0-6 ml. of dilute (1 5) hydrochloric acid and mixed with a few drops of starch solution if a blue (or blue-black) coloration appears in one minute, the test is positive. One convenient method of removing the peroxides is to reflux each one litre of recovered isopropyl alcohol with 10-15 g. of solid stannous chloride for half an hour. Test for peroxides with a portion of the cooled solution if iodine is liberated, add further 5 g. portions of stannous chloride followed by refluxing for half-hour periods until the test is negative. Then add about 200 g. of quicklime, reflux for 4 hours, and distil (Fig. II, 47, 2) discard the first portion of the distillate until the test for acetone is negative (Crotyl Alcohol, Note 1). Peroxides generally redevelop in tliis purified isopropyl alcohol in several days. 

In addition to the Review Exercises, sets of Exercises and Problems, and their solutions, are given at the end of eaeh seetion. 

Before moving on to the next section, it would be very useful to work some of the Exercises and Problems. In particular. Exercises 3, 5, and 12 as well as problems 6, 8, and 11 provide insight that would help when the material of the next section is studied. The solution to Problem 11 is used throughout this section to help illustrate the concepts introduced here. 

Potential health and safety problems of acryflc polymers occur in their manufacture (159). During manufacture, considerable care is exercised to reduce the potential for violent polymerizations and to reduce exposure to flammable and potentially toxic monomers and solvents. Recent environmental legislation governing air quality has resulted in completely closed ketde processes for most acryflc polymerizations. Acryflc solution polymers are treated as flammable mixtures. Dispersion polymers are nonflammable. 

An example of a commercial semibatch polymerization process is the early Union Carbide process for Dynel, one of the first flame-retardant modacryhc fibers (23,24). Dynel, a staple fiber that was wet spun from acetone, was introduced in 1951. The polymer is made up of 40% acrylonitrile and 60% vinyl chloride. The reactivity ratios for this monomer pair are 3.7 and 0.074 for acrylonitrile and vinyl chloride in solution at 60°C. Thus acrylonitrile is much more reactive than vinyl chloride in this copolymerization. In addition, vinyl chloride is a strong chain-transfer agent. To make the Dynel composition of 60% vinyl chloride, the monomer composition must be maintained at 82% vinyl chloride. Since acrylonitrile is consumed much more rapidly than vinyl chloride, if no control is exercised over the monomer composition, the acrylonitrile content of the monomer decreases to approximately 1% after only 25% conversion. The low acrylonitrile content of the monomer required for this process introduces yet another problem. That is, with an acrylonitrile weight fraction of only 0.18 in the unreacted monomer mixture, the low concentration of acrylonitrile becomes a rate-limiting reaction step. Therefore, the overall rate of chain growth is low and under normal conditions, with chain transfer and radical recombination, the molecular weight of the polymer is very low. 

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