Material Properties Archivy - Page 28 of 80

Sulfur and Potassium – Comparison – Properties

2021-01-13 by Nick Connor

This article contains comparison of key thermal and atomic properties of sulfur and potassium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Sulfur vs Potassium.

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Sulfur and Potassium – About Elements

Sulfur

Sulfur is abundant, multivalent, and nonmetallic. Under normal conditions, sulfur atoms form cyclic octatomic molecules with a chemical formula S8. Elemental sulfur is a bright yellow crystalline solid at room temperature. Chemically, sulfur reacts with all elements except for gold, platinum, iridium, tellurium, and the noble gases.

Potassium

Potassium was first isolated from potash, the ashes of plants, from which its name derives. In the periodic table, potassium is one of the alkali metals. All of the alkali metals have a single valence electron in the outer electron shell, which is easily removed to create an ion with a positive charge – a cation, which combines with anions to form salts. Naturally occurring potassium is composed of three isotopes, of which 40K is radioactive. Traces of 40K are found in all potassium, and it is the most common radioisotope in the human body.

Phosphorus in Periodic Table

Potassium in Periodic Table

Source: www.luciteria.com

Sulfur and Potassium – Applications

Sulfur

The greatest commercial use of the element is the production of sulfuric acid for sulfate and phosphate fertilizers, and other chemical processes. Sulfur is increasingly used as a component of fertilizers. The most important form of sulfur for fertilizer is the mineral calcium sulfate. The element sulfur is used in matches, insecticides, and fungicides. Many sulfur compounds are odoriferous, and the smells of odorized natural gas, skunk scent, grapefruit, and garlic are due to organosulfur compounds.

Potassium

Potassium (K) is an essential nutrient for plant growth. It’s classified as a macronutrient because plants take up large quantities of K during their life cycle. Agricultural fertilizers consume 95% of global potassium chemical production, and about 90% of this potassium is supplied as KCl. Due to its high degree of reactivity, pure potassium is rarely used in its elemental /metallic form. It is used as a powerful reducing agent in organic chemistry. Potassium/Sodium alloys are It used as a heat exchange medium . The heat in the potassium warms water and makes it hot enough to boil. Then water is changed into steam, which is used to work devices that generate electricity.

Sulfur and Potassium – Comparison in Table

Element	Sulfur	Potassium
Density	1.823 g/cm3	0.856 g/cm3
Ultimate Tensile Strength	N/A	N/A
Yield Strength	N/A	N/A
Young’s Modulus of Elasticity	N/A	3.53 GPa
Mohs Scale	0.5	0.4
Brinell Hardness	N/A	0.36 MPa
Vickers Hardness	N/A	N/A
Melting Point	44.1 °C	63.25 °C
Boiling Point	280 °C	760 °C
Thermal Conductivity	0.235 W/mK	102.4 W/mK
Thermal Expansion Coefficient	N/A	83 µm/mK
Specific Heat	0.77 J/g K	0.75 J/g K
Heat of Fusion	0.657 kJ/mol	2.334 kJ/mol
Heat of Vaporization	51.9 kJ/mol	79.87 kJ/mol

Sulfur and Chlorine – Comparison – Properties

2021-01-13 by Nick Connor

This article contains comparison of key thermal and atomic properties of sulfur and chlorine, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Sulfur vs Chlorine.

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Sulfur and Chlorine – About Elements

Sulfur

Chlorine

Chlorine is a yellow-green gas at room temperature. It is an extremely reactive element and a strong oxidising agent: among the elements, it has the highest electron affinity and the third-highest electronegativity, behind only oxygen and fluorine.

Phosphorus in Periodic Table

Chlorine in Periodic Table

Source: www.luciteria.com

Sulfur and Chlorine – Applications

Sulfur

Chlorine

Chlorine is used in the manufacture of a wide range of consumer products, about two-thirds of them organic chemicals such as polyvinyl chloride (PVC), many intermediates for the production of plastics, and other end products which do not contain the element. As a common disinfectant, elemental chlorine and chlorine-generating compounds are used more directly in swimming pools to keep them sanitary. While perhaps best known for its role in providing clean drinking water, chlorine chemistry also helps provide energy-efficient building materials, electronics, fiber optics, solar energy cells, 93 percent of life-saving pharmaceuticals, 86 percent of crop protection compounds, medical plastics, and much more.

Sulfur and Chlorine – Comparison in Table

Element	Sulfur	Chlorine
Density	1.823 g/cm3	0.0032 g/cm3
Ultimate Tensile Strength	N/A	N/A
Yield Strength	N/A	N/A
Young’s Modulus of Elasticity	N/A	N/A
Mohs Scale	0.5	N/A
Brinell Hardness	N/A	N/A
Vickers Hardness	N/A	N/A
Melting Point	44.1 °C	-101 °C
Boiling Point	280 °C	-34.6 °C
Thermal Conductivity	0.235 W/mK	0.0089 W/mK
Thermal Expansion Coefficient	N/A	N/A
Specific Heat	0.77 J/g K	0.48 J/g K
Heat of Fusion	0.657 kJ/mol	3.23 kJ/mol
Heat of Vaporization	51.9 kJ/mol	10.2 kJ/mol

Phosphorus and Magnesium – Comparison – Properties

2021-01-13 by Nick Connor

This article contains comparison of key thermal and atomic properties of phosphorus and magnesium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Phosphorus vs Magnesium.

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Phosphorus and Magnesium – About Elements

Phosphorus

As an element, phosphorus exists in two major forms—white phosphorus and red phosphorus—but because it is highly reactive, phosphorus is never found as a free element on Earth. At 0.099%, phosphorus is the most abundant pnictogen in the Earth’s crust.

Magnesium

Magnesium is a shiny gray solid which bears a close physical resemblance to the other five elements in the second column (group 2, or alkaline earth metals) of the periodic table: all group 2 elements have the same electron configuration in the outer electron shell and a similar crystal structure.

Phosphorus in Periodic Table

Magnesium in Periodic Table

Source: www.luciteria.com

Phosphorus and Magnesium – Applications

Phosphorus

Phosphorus is an essential plant nutrient (the most often limiting nutrient, after nitrogen), and the bulk of all phosphorus production is in concentrated phosphoric acids for agriculture fertilisers, containing as much as 70% to 75% P2O5. The vast majority of phosphorus compounds mined are consumed as fertilisers. Phosphate is needed to replace the phosphorus that plants remove from the soil, and its annual demand is rising nearly twice as fast as the growth of the human population. Other applications include organophosphorus compounds in detergents, pesticides, and nerve agents.

Magnesium

Magnesium is the third-most-commonly-used structural metal, following iron and aluminium.[35] The main applications of magnesium are, in order: aluminium alloys, die-casting (alloyed with zinc), removing sulfur in the production of iron and steel, and the production of titanium in the Kroll process. Magnesium alloys are used in a wide variety of structural and nonstructural applications. Structural applications include automotive, industrial, materials-handling, commercial, and aerospace equipment. Magnesium alloys are used for parts that operate at high speeds and thus must be light weight to minimize inertial forces. Commercial applications include hand-held tools, laptops, luggage, and ladders, automobiles (e.g., steering wheels and columns, seat frames, transmission cases). Magnox (alloy), whose name is an abbreviation for “magnesium non-oxidizing”, is 99% magnesium and 1% aluminum, and is used in the cladding of fuel rods in magnox nuclear power reactors.

Phosphorus and Magnesium – Comparison in Table

Element	Phosphorus	Magnesium
Density	1.823 g/cm3	1.738 g/cm3
Ultimate Tensile Strength	N/A	200 MPa
Yield Strength	N/A	N/A
Young’s Modulus of Elasticity	N/A	45 GPa
Mohs Scale	0.5	2.5
Brinell Hardness	N/A	260 MPa
Vickers Hardness	N/A	N/A
Melting Point	44.1 °C	649 °C
Boiling Point	280 °C	1090 °C
Thermal Conductivity	0.235 W/mK	156 W/mK
Thermal Expansion Coefficient	N/A	24.8 µm/mK
Specific Heat	0.77 J/g K	1.02 J/g K
Heat of Fusion	0.657 kJ/mol	8.954 kJ/mol
Heat of Vaporization	51.9 kJ/mol	127.4 kJ/mol

Phosphorus and Potassium – Comparison – Properties

2021-01-13 by Nick Connor

This article contains comparison of key thermal and atomic properties of phosphorus and potassium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Phosphorus vs Potassium.

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Phosphorus and Potassium – About Elements

Phosphorus

Potassium

Phosphorus in Periodic Table

Potassium in Periodic Table

Source: www.luciteria.com

Phosphorus and Potassium – Applications

Phosphorus

Potassium

Phosphorus and Potassium – Comparison in Table

Element	Phosphorus	Potassium
Density	1.823 g/cm3	0.856 g/cm3
Ultimate Tensile Strength	N/A	N/A
Yield Strength	N/A	N/A
Young’s Modulus of Elasticity	N/A	3.53 GPa
Mohs Scale	0.5	0.4
Brinell Hardness	N/A	0.36 MPa
Vickers Hardness	N/A	N/A
Melting Point	44.1 °C	63.25 °C
Boiling Point	280 °C	760 °C
Thermal Conductivity	0.235 W/mK	102.4 W/mK
Thermal Expansion Coefficient	N/A	83 µm/mK
Specific Heat	0.77 J/g K	0.75 J/g K
Heat of Fusion	0.657 kJ/mol	2.334 kJ/mol
Heat of Vaporization	51.9 kJ/mol	79.87 kJ/mol

Phosphorus and Calcium – Comparison – Properties

2021-01-13 by Nick Connor

This article contains comparison of key thermal and atomic properties of phosphorus and calcium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Phosphorus vs Calcium.

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Phosphorus and Calcium – About Elements

Phosphorus

Calcium

Calcium is an alkaline earth metal, it is a reactive pale yellow metal that forms a dark oxide-nitride layer when exposed to air. Its physical and chemical properties are most similar to its heavier homologues strontium and barium. It is the fifth most abundant element in Earth’s crust and the third most abundant metal, after iron and aluminium.

Phosphorus in Periodic Table

Calcium in Periodic Table

Source: www.luciteria.com

Phosphorus and Calcium – Applications

Phosphorus

Calcium

The largest use of metallic calcium is in steelmaking, due to its strong chemical affinity for oxygen and sulfur. Its oxides and sulfides, once formed, give liquid lime aluminate and sulfide inclusions in steel which float out. Calcium compounds are used as manufacture of insecticides, paints, blackboard chalk, textile and fireworks.

Phosphorus and Calcium – Comparison in Table

Element	Phosphorus	Calcium
Density	1.823 g/cm3	1.55 g/cm3
Ultimate Tensile Strength	N/A	110 MPa
Yield Strength	N/A	N/A
Young’s Modulus of Elasticity	N/A	20 GPa
Mohs Scale	0.5	1.5
Brinell Hardness	N/A	170 – 400 MPa
Vickers Hardness	N/A	N/A
Melting Point	44.1 °C	842 °C
Boiling Point	280 °C	1484 °C
Thermal Conductivity	0.235 W/mK	200 W/mK
Thermal Expansion Coefficient	N/A	22.3 µm/mK
Specific Heat	0.77 J/g K	0.63 J/g K
Heat of Fusion	0.657 kJ/mol	8.54 kJ/mol
Heat of Vaporization	51.9 kJ/mol	153.3 kJ/mol

Silicon and Copper – Comparison – Properties

2021-01-13 by Nick Connor

This article contains comparison of key thermal and atomic properties of silicon and copper, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Silicon vs Copper.

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Silicon and Copper – About Elements

Silicon

Silicon is a hard and brittle crystalline solid with a blue-grey metallic lustre, it is a tetravalent metalloid and semiconductor.

Copper

Copper is a soft, malleable, and ductile metal with very high thermal and electrical conductivity. A freshly exposed surface of pure copper has a reddish-orange color. Copper is used as a conductor of heat and electricity, as a building material, and as a constituent of various metal alloys, such as sterling silver used in jewelry, cupronickel used to make marine hardware and coins, and constantan used in strain gauges and thermocouples for temperature measurement.

Silicon in Periodic Table

Copper in Periodic Table

Source: www.luciteria.com

Silicon and Copper – Applications

Silicon

Most silicon is used industrially without being purified, and indeed, often with comparatively little processing from its natural form. Silicon is a vital ingredient in aluminum, steel, and iron alloys. It is added as a fluxing agent for copper alloys. In the form of clay and sand, it is used to manufacture bricks and concrete; it is a valuable refractory material for high-temperature work, for example, molding sands for castings in foundry applications. Silica is used to make fire brick, a type of ceramic. Silicate minerals are also in whiteware ceramics, an important class of products usually containing various types of fired clay minerals (natural aluminium phyllosilicates). An example is porcelain, which is based on the silicate mineral kaolinite. Traditional glass (silica-based soda-lime glass) also functions in many of the same ways, and also is used for windows and containers. Hyperpure silicon metal and doped hyperpure silicon (doping with boron, phosphorous, gallium, or arsenic) are used in solar cells, transistors and semiconductors.

Copper

Historically, alloying copper with another metal, for example tin to make bronze, was first practiced about 4000 years after the discovery of copper smelting, and about 2000 years after “natural bronze” had come into general use. An ancient civilization is defined to be in the Bronze Age either by producing bronze by smelting its own copper and alloying with tin, arsenic, or other metals. The major applications of copper are electrical wire (60%), roofing and plumbing (20%), and industrial machinery (15%). Copper is used mostly as a pure metal, but when greater hardness is required, it is put into such alloys as brass and bronze (5% of total use). Copper and copper-based alloys including brasses (Cu-Zn) and bronzes (Cu-Sn) are widely used in different industrial and societal applications. Some of the common uses for brass alloys include costume jewelry, locks, hinges, gears, bearings, ammunition casings, automotive radiators, musical instruments, electronic packaging, and coins. Bronze, or bronze-like alloys and mixtures, were used for coins over a longer period. is still widely used today for springs, bearings, bushings, automobile transmission pilot bearings, and similar fittings, and is particularly common in the bearings of small electric motors. Brass and bronze are common engineering materials in modern architecture and primarily used for roofing and facade cladding due to their visual appearance.

Silicon and Copper – Comparison in Table

Element	Silicon	Copper
Density	2.33 g/cm3	8.92 g/cm3
Ultimate Tensile Strength	170 MPa	210 MPa
Yield Strength	165 MPa	33 MPa
Young’s Modulus of Elasticity	150 GPa	120 GPa
Mohs Scale	7	3
Brinell Hardness	2300 MPa	250 MPa
Vickers Hardness	N/A	350 MPa
Melting Point	1410 °C	1084.62 °C
Boiling Point	3265 °C	2562 °C
Thermal Conductivity	148 W/mK	401 W/mK
Thermal Expansion Coefficient	2.6 µm/mK	16.5 µm/mK
Specific Heat	0.71 J/g K	0.38 J/g K
Heat of Fusion	50.55 kJ/mol	13.05 kJ/mol
Heat of Vaporization	384.22 kJ/mol	300.3 kJ/mol

Silicon and Germanium – Comparison – Properties

2021-01-13 by Nick Connor

This article contains comparison of key thermal and atomic properties of silicon and germanium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Silicon vs Germanium.

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Silicon and Germanium – About Elements

Silicon

Silicon is a hard and brittle crystalline solid with a blue-grey metallic lustre, it is a tetravalent metalloid and semiconductor.

Germanium

Germanium is a lustrous, hard, grayish-white metalloid in the carbon group, chemically similar to its group neighbors tin and silicon. Pure germanium is a semiconductor with an appearance similar to elemental silicon.

Silicon in Periodic Table

Germanium in Periodic Table

Source: www.luciteria.com

Silicon and Germanium – Applications

Silicon

Germanium

In gamma spectroscopy, germanium is preferred due to its atomic number being much higher than silicon and which increases the probability of gamma ray interaction. Moreover, germanium has lower average energy necessary to create an electron-hole pair, which is 3.6 eV for silicon and 2.9 eV for germanium. This also provides the latter a better resolution in energy. A large, clean and almost perfect germanium semiconductor is ideal as a counter for radioactivity. However, it is difficult and expensive to make large crystals with sufficient purity. On the other hand, in order to achieve maximum efficiency the detectors must operate at the very low temperatures of liquid nitrogen (-196°C), because at room temperatures the noise caused by thermal excitation is very high. Since germanium detectors produce the highest resolution commonly available today, they are used to measure radiation in a variety of applications including personnel and environmental monitoring for radioactive contamination, medical applications, radiometric assay, nuclear security and nuclear plant safety.

Silicon and Germanium – Comparison in Table

Element	Silicon	Germanium
Density	2.33 g/cm3	5.323 g/cm3
Ultimate Tensile Strength	170 MPa	135 MPa
Yield Strength	165 MPa	135 MPa
Young’s Modulus of Elasticity	150 GPa	103 GPa
Mohs Scale	7	6
Brinell Hardness	2300 MPa	N/A
Vickers Hardness	N/A	N/A
Melting Point	1410 °C	938.3 °C
Boiling Point	3265 °C	2820 °C
Thermal Conductivity	148 W/mK	59.9 W/mK
Thermal Expansion Coefficient	2.6 µm/mK	6 µm/mK
Specific Heat	0.71 J/g K	0.32 J/g K
Heat of Fusion	50.55 kJ/mol	36.94 kJ/mol
Heat of Vaporization	384.22 kJ/mol	330.9 kJ/mol

Silicon and Arsenic – Comparison – Properties

2021-01-13 by Nick Connor

This article contains comparison of key thermal and atomic properties of silicon and arsenic, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Silicon vs Arsenic.

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Silicon and Arsenic – About Elements

Silicon

Silicon is a hard and brittle crystalline solid with a blue-grey metallic lustre, it is a tetravalent metalloid and semiconductor.

Arsenic

Arsenic occurs in many minerals, usually in combination with sulfur and metals, but also as a pure elemental crystal. Arsenic is a metalloid.

Silicon in Periodic Table

Arsenic in Periodic Table

Source: www.luciteria.com

Silicon and Arsenic – Applications

Silicon

Arsenic

Arsenic is used as a doping agent in semiconductors (gallium arsenide) for solid-state devices. It is also used in bronzing, pyrotechnics and for hardening shot. Arsenic compounds can be used to make special glass and preserve wood.

Silicon and Arsenic – Comparison in Table

Element	Silicon	Arsenic
Density	2.33 g/cm3	5.727 g/cm3
Ultimate Tensile Strength	170 MPa	N/A
Yield Strength	165 MPa	N/A
Young’s Modulus of Elasticity	150 GPa	8 GPa
Mohs Scale	7	3.5
Brinell Hardness	2300 MPa	1440 MPa
Vickers Hardness	N/A	N/A
Melting Point	1410 °C	817 °C
Boiling Point	3265 °C	614 °C
Thermal Conductivity	148 W/mK	50 W/mK
Thermal Expansion Coefficient	2.6 µm/mK	5.6 µm/mK
Specific Heat	0.71 J/g K	0.33 J/g K
Heat of Fusion	50.55 kJ/mol	N/A
Heat of Vaporization	384.22 kJ/mol	34.76 kJ/mol

Aluminium and Gallium – Comparison – Properties

2021-01-11 by Nick Connor

This article contains comparison of key thermal and atomic properties of aluminium and gallium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Aluminium vs Gallium.

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Aluminium and Gallium – About Elements

Aluminium

Aluminium is a silvery-white, soft, nonmagnetic, ductile metal in the boron group. By mass, aluminium makes up about 8% of the Earth’s crust; it is the third most abundant element after oxygen and silicon and the most abundant metal in the crust, though it is less common in the mantle below.

Gallium

Gallium has similarities to the other metals of the group, aluminium, indium, and thallium. Gallium does not occur as a free element in nature, but as gallium(III) compounds in trace amounts in zinc ores and in bauxite.

Aluminium in Periodic Table

Gallium in Periodic Table

Source: www.luciteria.com

Aluminium and Gallium – Applications

Aluminium

Aluminium and its alloys are used widely in aerospace, automotive, architectural, lithographic, packaging, electrical and electronic applications. It is the prime material of construction for the aircraft industry throughout most of its history. About 70% of commercial civil aircraft airframes are made from aluminium alloys, and without aluminium civil aviation would not be economically viable. Automotive industry now includes aluminium as engine castings, wheels, radiators and increasingly as body parts. 6111 aluminium and 2008 aluminium alloy are extensively used for external automotive body panels. Cylinder blocks and crankcases are often cast made of aluminium alloys.

Gallium

Gallium consumption is centred on the superconductor industry. Semiconductor applications dominate the commercial demand for gallium, accounting for 98% of the total. When alloyed with arsenic to produce gallium arsenide (GaAs), it can convert electricity to light. Due to such properties, it is used in LEDs, and has been found to produce less heat than silicon, rendering it suitable for use in supercomputers.

Aluminium and Gallium – Comparison in Table

Element	Aluminium	Gallium
Density	2.7 g/cm3	5.904 g/cm3
Ultimate Tensile Strength	90 MPa (pure), 600 MPa (alloys)	15 MPa
Yield Strength	11 MPa (pure), 400 MPa (alloys)	8 MPa
Young’s Modulus of Elasticity	70 GPa	9.8 GPa
Mohs Scale	2.8	1.5
Brinell Hardness	240 MPa	60 MPa
Vickers Hardness	167 MPa	N/A
Melting Point	660 °C	29.76 °C
Boiling Point	2467 °C	2204 °C
Thermal Conductivity	237 W/mK	40.6 W/mK
Thermal Expansion Coefficient	23.1 µm/mK	18 µm/mK
Specific Heat	0.9 J/g K	0.37 J/g K
Heat of Fusion	10.79 kJ/mol	5.59 kJ/mol
Heat of Vaporization	293.4 kJ/mol	258.7 kJ/mol

Aluminium and Iron – Comparison – Properties

2021-01-11 by Nick Connor

This article contains comparison of key thermal and atomic properties of aluminium and iron, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Aluminium vs Iron.

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Aluminium and Iron – About Elements

Aluminium

Iron

Iron is a metal in the first transition series. It is by mass the most common element on Earth, forming much of Earth’s outer and inner core. It is the fourth most common element in the Earth’s crust. Its abundance in rocky planets like Earth is due to its abundant production by fusion in high-mass stars.

Aluminium in Periodic Table

Iron in Periodic Table

Source: www.luciteria.com

Aluminium and Iron – Applications

Aluminium

Iron

Iron is used in numerous sectors such as electronics, manufacturing, automotive, and construction and building. Iron is the most widely used of all the metals, accounting for over 90% of worldwide metal produc0tion. Its low cost and high strength often make it the material of choice material to withstand stress or transmit forces, such as the construction of machinery and machine tools, rails, automobiles, ship hulls, concrete reinforcing bars, and the load-carrying framework of buildings. Since pure iron is quite soft, it is most commonly combined with alloying elements to make steel. Steels are iron–carbon alloys that may contain appreciable concentrations of other alloying elements. Adding a small amount of non-metallic carbon to iron trades its great ductility for the greater strength. Due to its very-high strength, but still substantial toughness, and its ability to be greatly altered by heat treatment, steel is one of the most useful and common ferrous alloy in modern use. There are thousands of alloys that have different compositions and/or heat treatments. The mechanical properties are sensitive to the content of carbon, which is normally less than 1.0 wt%.

Aluminium and Iron – Comparison in Table

Element	Aluminium	Iron
Density	2.7 g/cm3	7.874 g/cm3
Ultimate Tensile Strength	90 MPa (pure), 600 MPa (alloys)	540 MPa
Yield Strength	11 MPa (pure), 400 MPa (alloys)	50 MPa
Young’s Modulus of Elasticity	70 GPa	211 GPa
Mohs Scale	2.8	4.5
Brinell Hardness	240 MPa	490 MPa
Vickers Hardness	167 MPa	608 MPa
Melting Point	660 °C	1538 °C
Boiling Point	2467 °C	2861 °C
Thermal Conductivity	237 W/mK	80.2 W/mK
Thermal Expansion Coefficient	23.1 µm/mK	11.8 µm/mK
Specific Heat	0.9 J/g K	0.44 J/g K
Heat of Fusion	10.79 kJ/mol	13.8 kJ/mol
Heat of Vaporization	293.4 kJ/mol	349.6 kJ/mol