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Acetylene, the Principles of Its Generation and Use: A Practical Handbook on the Production, Purification, and Subsequent Treatment of Acetylene for the Development of Light, Heat, and PowerLeeds, F. H. (Frank Henley)

Science

Acetylene, the Principles of Its Generation and Use: A Practical Handbook on the Production, Purification, and Subsequent Treatment of Acetylene for the Development of Light, Heat, and Power

Name: Acetylene, the Principles of Its Generation and Use: A Practical Handbook on the Production, Purification, and Subsequent Treatment of Acetylene for the Development of Light, Heat, and Power
Author: Leeds, F. H. (Frank Henley)

Leeds, F. H. (Frank Henley)

Acetylene

It appears from this table that, with the exception of the three
hydrocarbons last named, no substance likely to be formed by the action
of heat on acetylene has nearly so high an illuminative value--volume for
volume--as acetylene itself. The richly illuminating vapours of benzene
and naphthalene (and homologues) cannot practically add to the
illuminative value of acetylene, because of the difficulty of consuming
them without smoke, unless they are diluted with a large proportion of
feebly- or non-illuminating gas, such as methane or hydrogen. The
practical effect of carburetting acetylene with hydrocarbon vapours will
be shown in Chapter X. to be disastrous so far as the illuminating
efficiency of the gas is concerned. Hence it appears that no conceivable
products of the polymerisation of acetylene by heat can result in its
illuminative value being improved--even presupposing that the burners
could consume the polymers properly--while practically a considerable
deterioration of its value must ensue.

The heat of combustion of acetylene was found by J. Thomson to be 310.57
large calories per gramme-molecule, and by Berthelot to be 321.00
calories. The latest determination, however, made by Berthelot and
Matignon shows it to be 315.7 calories at constant pressure. Taking the
heat of formation of carbon dioxide from diamond carbon at constant
pressure as 94.3 calories (Berthelot and Matignon), which is equal to
97.3 calories from amorphous carbon, and the heat of formation of liquid
water as 69 calories; this value for the heat of combustion of acetylene
makes its heat of formation to be 94.3 x 2 + 69 - 315.7 = -58.1 large
calories per gramme-molecule (26 grammes) from diamond carbon, or -52.1
from amorphous carbon. It will be noticed that the heat of combustion of
acetylene is greater than the combined heats of combustion of its
constituents; which proves that heat has been absorbed in the union of
the hydrogen and carbon in the molecule, or that acetylene is
endothermic, as elsewhere explained. These calculations, and others given
in Chapter IX., will perhaps be rendered more intelligible by the
following table of thermochemical phenomena:

Public-domain text, read in full here on John Shaqi.

Opening the text

Science

Acetylene, the Principles of Its Generation and Use: A Practical Handbook on the Production, Purification, and Subsequent Treatment of Acetylene for the Development of Light, Heat, and Power

Leeds, F. H. (Frank Henley)

Acetylene

It appears from this table that, with the exception of the three
hydrocarbons last named, no substance likely to be formed by the action
of heat on acetylene has nearly so high an illuminative value--volume for
volume--as acetylene itself. The richly illuminating vapours of benzene
and naphthalene (and homologues) cannot practically add to the
illuminative value of acetylene, because of the difficulty of consuming
them without smoke, unless they are diluted with a large proportion of
feebly- or non-illuminating gas, such as methane or hydrogen. The
practical effect of carburetting acetylene with hydrocarbon vapours will
be shown in Chapter X. to be disastrous so far as the illuminating
efficiency of the gas is concerned. Hence it appears that no conceivable
products of the polymerisation of acetylene by heat can result in its
illuminative value being improved--even presupposing that the burners
could consume the polymers properly--while practically a considerable
deterioration of its value must ensue.

The heat of combustion of acetylene was found by J. Thomson to be 310.57
large calories per gramme-molecule, and by Berthelot to be 321.00
calories. The latest determination, however, made by Berthelot and
Matignon shows it to be 315.7 calories at constant pressure. Taking the
heat of formation of carbon dioxide from diamond carbon at constant
pressure as 94.3 calories (Berthelot and Matignon), which is equal to
97.3 calories from amorphous carbon, and the heat of formation of liquid
water as 69 calories; this value for the heat of combustion of acetylene
makes its heat of formation to be 94.3 x 2 + 69 - 315.7 = -58.1 large
calories per gramme-molecule (26 grammes) from diamond carbon, or -52.1
from amorphous carbon. It will be noticed that the heat of combustion of
acetylene is greater than the combined heats of combustion of its
constituents; which proves that heat has been absorbed in the union of
the hydrogen and carbon in the molecule, or that acetylene is
endothermic, as elsewhere explained. These calculations, and others given
in Chapter IX., will perhaps be rendered more intelligible by the
following table of thermochemical phenomena:

Public-domain text, read in full here on John Shaqi.

Acetylene, the Principles of Its Generation and Use: A Practical Handbook on the Production, Purification, and Subsequent Treatment of Acetylene for the Development of Light, Heat, and Power

Acetylene, the Principles of Its Generation and Use: A Practical Handbook on the Production, Purification, and Subsequent Treatment of Acetylene for the Development of Light, Heat, and Power

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