Chemistry conversion factors

Formulas, Molecular and Equivalent Weights, and Conversion Factors to CaCO, of Substances Frequently Appearing in the Chemistry of Water Softening... 

Conversion Factors to CaCOj of Substances Frequentl Appearing in the Chemistry of Water Softening y MitUipItfi/iff Factor Conail, of CitCOi na 100. ... 

Conversion Factors to CaCOj of Substances Frequently Appearing in die Chemistry of Water Softmiing MiUlipljting Factor CoasfdcWnp vnotoculor wt, of CuCOi at too. ... 

Molar mass can be thought of as a conversion factor between mass in grams and number of moles. These conversions are essential in chemistry, because chemists count amounts of substances in moles but routinely... 

The use of non-SI units is strongly discouraged. For these units there often do not exist standards, and for historical reasons the same denomination may mean sundry units. For example, it is common practice in theoretical chemistry to state energy values in kilocalories. However, to convert a calorie to the SI unit Joule, there exist different conversion factors ... 

A number of non-SI units are commonly used in the literature of quantum chemistry. We therefore provide appropriate conversion factors for certain specialized units used in this chapter ... 

Calculated from Ionization potentials of atoms and atomic ions in the CRC Handbook of Chemistry and Physics [8] Conversion factor 1 hartree = 27.2114 eV... 

As with many things in life, chemistry isn t always as easy as it seems. Chemistry teachers are sneaky They often give you quantities in non-Sl units and expect you to use one or more conversion factors to change them to SI units — all this before you even attempt the hard part of the problem We re at least mcirginally less sneaky than your typical chemistry teacher, but we hope to prepare you for such deception, so expect to use conversion factors throughout the rest of this book ... 

Before you start your hooray-chemistry-is-finally-getting-simple dance, understand that certain conditions apply to this conversion factor. For example, it s true only at standard temperature and pressure (STP), or 0°C and 1 atmosphere. Also, the figure of 22.4 L/mol applies only to the extent that a gas resembles an ideal gas, one whose particles have zero volume and neither attract nor repel one another. Ultimately, no gas is truly ideal, but many are so close to being so that the 22.4 L/mol conversion is very useful. 

From these nine basic quantities, numerous other SI units may be derived. Table B.2 lists a number of these derived units, particularly those relevant to colloid and surface chemistry. The table is arranged alphabetically according to the name of the physical quantity involved. Note that instructions for the use of the conversion factors —depending on the direction of the conversion —are given in the top and bottom headings of the columns. Table B.2 is by no means an exhaustive list of the various derived SI units Hopkins (1973) reports on many additional conversions, as do most handbooks and numerous other references. 

Often in chemistry, and especially in a laboratory setting, it is necessary to convert from one unit to another. To do so, you need only multiply the given quantity by the appropriate conversion factor All conversion factors can be written as ratios in which the numerator and denominator represent the equivalent quantity expressed in different units. Because any quantity divided by itself is equal to i, all conversion factors are equal to i. For example, the following two conversion factors are both derived from the relationship ioo centimeters = i meter ... 

Instructors can cover as much of the Fundamentals as they wish, whenever they wish skip it all or assign it for independent study. Students can also turn to the Appendixes for help with mathematics, units, conversion factors, and the correct use—within the normal practice of general chemistry, at least—of significant figures. 

Because virtually all stoichiometric calculations involve moles (abbreviated mol) of material, molarity is probably the most common concentration unit in chemistry. If we dissolved 1.0 mol of glucose in enough water to give a total volume of 1.0 L, we would obtain a 1.0 molar solution of glucose. Molarity is abbreviated with a capital M. Notice that, because molarity has units of moles per liter, molar concentrations are conversion factors between moles of material and liters of solution. 

In this unit you will find explanations, examples, and practice dealing with the calculations encountered in the chemistry discussed in this book. The types of calculations included here involve conversion factors, metric use, algebraic manipulations, scientific notation, and significant figures. This unit can be used by itself or be incorporated for assistance with individual units. Unless otherwise noted, all answers are rounded to the hundredth place. The calculator used here is a Casio FX-260. Any calculator that has a log (logarithm) key and an exp (exponent) key is sufficient for these chemical calculations. 

Section 7.1 gives examples illustrating the use of quantity calculus for converting the values of physical quantities between different units. The table in section 7.2 lists a variety of non-SI units used in chemistry, with the conversion factors to the corresponding SI units. Conversion factors for energy and energy-related units (wavenumber, frequency, temperature and molar energy), and for pressure units, are also presented in tables inside the back cover. 

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. 

For the foreseeable future, you will need to make conversions from other units to SI units, as much of the literature quotes data using imperial, c.g.s. or other systems. You will need to recognize these units and find the conversion factors required. Examples relevant to chemistry are given in Box 9.1. Table 9.4 provides values of some important physical constants in SI units. 

In chemistry, you often need to convert a measurement from one unit to another. One way of doing this is to use a conversion factor. A conversion factor is a simple ratio that relates two units that express a measurement of the same quantity. Conversion factors are formed by setting up a fraction that has equivalent amounts on top and bottom. For example, you can construct conversion factors between kilograms and grams as follows ... 

Now, suppose that while working in chemistry lab, you need 3.00 moles of manganese (Mn) for a chemical reaction. How can you measure that amount Like the 5 dozen jellybeans, the number of moles of manganese can be converted to an equivalent mass and measured on a balance. To calculate mass from the number of moles, you need to multiply the number of moles of manganese required in the reaction (3.00 moles of Mn) by a conversion factor that relates mass and moles of manganese. That conversion factor is the molar mass of manganese (54.9 g/mol). 

You make unit conversions everyday when you determine how many quarters are needed to make a dollar or how many feet are in a yard. One unit that is often used in calculations in chemistry is the mole. Chapter 11 shows you equivalent relationships among mole, grams, and the number of representative particles (atoms, molecules, formula units, or ions). For example, one mole of a substance contains 6.02 X 10 representative particles. Try the next example to see how this information can be used in a conversion factor to determine the number of atoms in a sample of manganese. 

In Lesson 2-11 told you that the liter is an outdated unit, but the truth is that it continues to be useful in chemistry class. In your laboratory, you can find graduated cylinders, beakers, and flasks that measure volume in liters and milliliters. To convert between the liter and the more accepted units of cubed lengths, try to commit the following conversion factors to memory. 

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