VAPOR DENSITY AND MOLECULAR WEIGHT.
Examine a liter measure, in the form of a cube,--cubic decimeter,
--and a cubic centimeter.
171. Gaseous Weights and Volumes.--A liter of H, at 0 degrees
and 760 mm., weighs nearly 0.09 g. This weight is called a crith.
Find the weight of H in the following, in criths and in grams: 15
1., 0.07 1., 50.3 1., 0.035 1., 0.6 1..
It has been estimated that there are (10) 24. molecules of H in a
liter. Does the number vary for different gases? The weight of a
molecule of H in parts of a crith is 1/(10) 24.; in parts of a
gram .09/(10) 24.. If the H molecule is composed of 2 atoms, what
is the weight of its atom in fractions of a crith? What in
fractions of a gram? The weight of the H atom is a microcrith.
What part of a crith is a microcrith?
172. Vapor Density.--Vapor density, or specific gravity referred
to H as the standard, (Physics) is the ratio of the weight of a
given volume of a gas or vapor to the weight of the same volume
of H. A liter of steam weighs nine times as much as a liter of H.
Its vapor density is therefore nine. For convenience, a definite
volume of H is usually taken as the standard, viz., the H atom.
The volume of the H atom and that of the half-molecule of H2O, or
of any gas are identical, each being represented by one square.
If, then, the standard of vapor density is the H atom, half the
molecular weight of a gas must be its vapor density, since it is
evident that we thus compare the weights of equal volumes. The
vapor density of H2O, steam, is found from the symbol as follows:
(2 + 16) / 2 = 9. To obtain the vapor density of any compound
from the formula, we have only to divide its molecular weight by
two. Find the vapor density of HCl, N2O, NO, C12H22O11, Cl, CO2,
HF, SO2. Explain each case.
The half-molecule, instead of the whole, is taken; because our
standard is the hydrogen atom, the smallest portion of matter, by
weight, known to science.
How many criths in a liter of HCl? How many grams? Compute the
number of criths and of grams in one liter of the compounds whose
symbols appear above.
PROBLEMS.
(1) A certain volume of H weighs 0.36 g. at standard temperature
and pressure. How many liters does it contain? If one liter
weighs 0.09 g., to weigh 0.36 g. it will take 0.36 / 0.09 = 4
liters.
(2) How many liters, or criths, of H in 63 g.? 2.7 g.? 1 g.? 5
g.? 250 g.? Explain each.
(3) Suppose the gas to be twice as heavy as H, how many liters in
0.36 g.? A liter of the gas will weigh 0.18 g. (0.09 X 2). In
0.36 g. there will be 0.36 / 0.18 = 2. Answer the question for 63
g., 2.7 g., etc.
(4) How many liters of Cl in each of the above numbers of grams?
(5) How many of HCl? H2O (steam)? CO2? Explain fully every case.
Vapor density is very easily determined from the formula by the
method given above. But in practice the formula is obtained from
the vapor density, and hence the method there given has to be
reversed.
173. Vapor Density of Oxygen.--Suppose we were to obtain the
vapor density of O. We should carefully seal and weigh a given
volume, say a liter, at a noted temperature and barometric
pressure, which are reducedto 0 degrees and 760 mm, and compare
it with the weight of the same volume of H. This has been done
repeatedly, and O has been found to weigh 16 times as much as H,
volume for volume, or, more exactly, 15.96+. Now a liter of each
gas has the same number of molecules, therefore the O molecule
weighs 16 times the H molecule. The half-molecule of each has the
same proportion, and the vapor density of O is 16. Atomic weight
is obtained in a very different way.
PROBLEMS.
(1) A liter of Cl is found to weigh 3.195 g. Compute its vapor
density, and explain fully.
(2) A liter of Hg vapor, under standard conditions, weighs 9 g.
Find its vapor density, and explain.
The vapor density of only a few elements has been satisfactorily
determined. See page 12. Some cannot be vaporized; others can be,
but only under conditions which prevent weighing them. The vapor
density of very many compounds also is unknown.
(3) A liter of CO2 weighs 1.98 g. Find the vapor density, and
from that the molecular weight, remembering that the latter is
twice the former. See whether it corresponds to that obtained
from the formula, CO2. This is,in fact, the way a formula is
ascertained, if the atomic weights of its elements are known.
(4) A liter of a compound gas weighs 2.88 g. Analysis shows that
its weight is half S and half O. As the atomic weight of S is 32,
and that of O is 16, what is the symbol for the gas?
Solution. Its molecular weight is 64, i.e. (2.88=0.09) X 2, of
which 32 is S and 32 O. The atomic weight of S is 32, hence there
is one atom of S, while of O there are two atoms. The formula is
SO2.
(5) A liter of a compound gas, which is found to contain 1 C and
3 O by weight, weighs 1.26 g. What is its formula? Atomic weights
are taken from page 12. Prove your answer.
(6) A liter of a compound of N and O weighs 1.98 g. The N is
7/11; and the O 4/11. What is the gas?
(7) A compound of N and H gas weighs 0.765 g. to the liter. The N
is 14/17 of the whole, the H 3/17. What gas is it? CHAPTER XXXV.
ATOMIC WEIGHT.
174. Definition.--We have seen that the molecular weight of a
compound, as well as of most elements, is obtained from the vapor
density by doubling the latter. It remains to explain how atomic
weights are obtained. The term is rather misleading. The atomic
weight of an element is its least combining weight, the smallest
portion that enters into chemical union, which is, of course, the
weight of an atom.
175. Atomic Weight of Oxygen.--Suppose we wish to find the atomic
weight of oxygen. We must find the smallest proportion by weight
in which it occurs in any compound. This can only be done by
analyzing all the compounds of O that can be vaporized. As
illustrative of these compounds take the six following:--
Wt. of other
Names. V. d. Mol. Wt. Wt. of O. Elem. Symbol.
Carbon monoxide... 14 28 16 12 ?
Carbon dioxide.... 22 44 32 12 ?
Hydrogen monoxide... 9 18 16 2 ?
Nitrogen monoxide... 22 44 16 28 ?
Nitrogen trioxide... 38 76 48 28 ?
Nitrogen pentoxide... 54 108 80 28 ?
176. Molecular Symbols.--From the vapor density of the gases--
column 2--we obtain their molecular weight-- column 3. To find
the proportion of O, it must be separated by chemical means from
its compounds and separately weighed. These relative weights are
given in column 4. Now the smallest weight of O which unites in
any case is its atomic weight. If any compound of O should in
future be found in which its combining weight is 8 or 4, that
would be called its atomic weight. By dividing the numbers in
column 4, wt. of O, by 16, the atomic weight of O, we obtain the
number of O atoms in the molecule. Subtracting the weights of O
from the molecular weights, we have the parts of the other
elements, column 5, and dividing these by the atomic weight of
the respective elements, we have the number of atoms of those
elements, these last, combined with the number of O atoms, give
the symbol. In this way complete the last column.
Show how to get the atomic weight of Cl from these compounds,
arranging them in tabular form, and completing as above: HCl,
KCl, NaCl, ZnCl2, MgCl2; the atomic weight of N in these: N2O,
NO, NH3.
177. Molecular and Atomic Volumes.--We thus see that vapor
density and atomic weight are obtained in two quite different
ways. In the case of elements the two are usually identical, i.e.
with the few whose vapor density is known; but this is not always
true, and it leads to interesting conclusions regarding atomic
volume. In O both vapor density and atomic weight are 16. This
gives 2 atoms of O to the molecule, i.e. the molecular weight /
the atomic weight. The size of an O atom is therefore half the
gaseous molecule, and is represented by one square. S has a vapor
density and an atomic weight of 32 each. Compute the number of
atoms in the molecule. Compute for I, in which the two are
identical, 127. P has an atomic weight of 31, while its vapor
density is 62. Its molecule must consist of 4 atoms, each half
the size of the H atom, The vapor density of As is 150, the
atomic weight 75. Compute the number of atoms in its molecule,
and represent their relative size. Hg has an atomic weight of
200, a vapor density of 100. Compute as before, and compare the
results with those on page 12. Ozone has an atomic weight of 16,
a vapor density 24. Compute.