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Solids liquids gas basics of investing

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Statistical Thermodynamics Specialization. Advanced Level. Hours to complete. Available languages. Daily Professor Mechanical Engineering. Offered by. University of Colorado Boulder CU-Boulder is a dynamic community of scholars and learners on one of the most spectacular college campuses in the country. Syllabus - What you will learn from this course. Week 1. Video 4 videos. Property Relations including the Virial Equation of State 4m.

Potential Energy Functions 5m. Empirical Equations of States 4m. Reading 4 readings. Property Relations including the Virial Equation of State 10m. Potential Energy Functions 10m. Empirical Equations of State 10m. Week 2. Video 3 videos. The Basics of Thermodynamic Stability 6m. Gibb's Phase Rule 4m. Reading 3 readings. The Basics of Thermodynamic Stability 10m.

Gibb's Phase Rule 10m. Quiz 1 practice exercise. Week 3. Molecular Dynamics 7m. Determining g r from Molecular Dynamics 4m. Molecular Dynamics 10m. Determining g r from Molecular Dynamics 10m. Week 4. Video 2 videos. Solids: The Einstein Crystal 6m. The Debye Crystal 6m. Reading 2 readings. Solids and the Einstein Crystal 10m. The Debye Crystal 10m. Quiz 3 practice exercises. Reviews 4. About the Statistical Thermodynamics Specialization.

Frequently Asked Questions When will I have access to the lectures and assignments? If you don't see the audit option: The course may not offer an audit option. You can try a Free Trial instead, or apply for Financial Aid. The course may offer 'Full Course, No Certificate' instead. This option lets you see all course materials, submit required assessments, and get a final grade. This also means that you will not be able to purchase a Certificate experience. What will I get if I subscribe to this Specialization?

Is financial aid available? Under favourable conditions, when they were quickly covered by sediment and thus sheltered from oxygen, preventing rot, these were converted to thick layers of coal. In some places, the hydrocarbons came into contact with bacteria with an appetite for certain molecules, which changed their composition.

So each reservoir storing accumulated solar energy will have its own character in terms of reservoir shape and hydrocarbon composition. Over time, we humans have developed a great hunger for energy. Originally, this was fulfilled by firewood.

But the solid form of coal was cumbersome, dangerous to dig up and not very economical. Eventually, oil reservoirs were discovered. Later, wells were drilled especially in the Middle East, where vast resources of fairly easily extractable oil appeared to be situated under the sand. The combustion engine caused an explosive growth in the demand for oil.

This grew so quickly that the end of the supply seemed near. The Club of Rome, a global think tank for political issues, warned that mankind was quickly running out of energy reserves. So people started to search in more inaccessible places and discovered much more oil under water: the North Sea, the Gulf of Mexico, the Niger Delta in Nigeria.

Driven by high oil prices, technology was developed to recover oil from increasingly deep water. Moreover, natural gas came into view. Originally, striking gas on a drill was considered bad luck. Locally, you may have been able to use it, but exporting it over long distances was far too expensive. Here too, technological developments changed the situation. Recently, it also became possible to chemically transform gas on a commercial scale to heavier liquid hydrocarbons such as gasoline or diesel fuel GtL, gas to liquid.

Thus, huge gas reserves in the Persian Gulf, for example, there is a reservoir 10 times as large as Slochteren in the Netherlands, the largest European natural gas field, estimated at 1. All this was possible thanks to the development of highly advanced technology. The first oil well for Shell in Malaysia, in Miri, was only m deep, and was drilled in with a technique that the Chinese had used for centuries to drill for salt. In the 60 years of its existence, m 3 of oil were retrieved by a pumpjack.

Today, oil is extracted from reserves in up to 2. This requires the precise drilling of a 6 km deep, 50 cm diameter hole from a drilling platform bobbing a few kilometres higher up on the sea. Then, at the bottom of the sea, a construction called a subsea well head has to be placed on the well, from which the oil must flow to a production platform which sometimes lies dozens of kilometres away.

This is not to be confused with the drilling platform, which drills and constructs the wells and then goes away. Production platforms instead contain the processing equipment. Between the reservoir and the platform, a multitude of problems can occur which must be known and mastered. Cost per kWh: The cost depends enormously on the source. Production costs range from a handful of dollars per barrel for easy oil in Saudi Arabia to tens of dollars per barrel for heavy oil in remote locations.

Risks: Pollution during transport and production; CO 2 production when used. Estimated research time: Research will be done for as long as these fuels exist, to make them cheaper, cleaner and more energy efficient, to extract a greater fraction of oil from a reservoir e.

One thing is clear: all the oil or gas that has been pumped out is gone forever. Slochteren is running out, the famous North Sea fields are running out, and even in the Gulf of Mexico, the most important oil source for the most energy-hungry country in the world — the USA — the fields being found are increasingly small.

Will the hydrocarbon economy soon die a slow, or perhaps a quick, death? Ultimately, supplies are certainly finite, but there are still a few aces up the hydrocarbon sleeve. Depending on the precise circumstances of an oil reservoir, approximately one-third of the available oil is generally extracted. The rest stays behind in the pores of the rock. Using technology, something can still be done to extract more oil: from relatively simple water injection to press the oil from the reservoir, to sweeps with surfactants and polymers to loosen some of the oil from the rock.

Thanks to high oil prices, these enhanced oil recovery techniques are becoming very interesting. There are also reservoirs which contain very heavy, i. Previously, these were not economically developed, but here too, technology can bring about change. But it is not easy and will require large investments, also in knowledge building.

Hyperheavy oil is still in abundance. In Canada, m 3 of oil are produced daily from excavated tar sands. This is a costly and difficult process, if only because of the extremely low temperatures that prevail in that region. Moreover, the process of producing useful fluids from oil sands requires quite a bit of energy and is not so efficient. Coal reserves are still in abundance, too. In recent years, coal has been the fastest growing energy source. This is because of the growing economy — and consequent demand for energy — in China, which itself has only limited oil and gas reserves, but a lot of coal.

But this is not without its price: the deaths of dozens of miners per day! With modern processes such as transformation of coal to gas it is possible to produce energy from coal in a less environmentally damaging way. And with more money and less haste, the safety situation can also be improved. Methane, of bacterial or fossil origin, which is released at the bottom of the sea, can form what are known as gas hydrates.

This is a kind of ice which, due to methane trapped inside under pressure , has a higher melting point. Great quantities of methane are likely to be stored in such huge hydrate fields at the bottom of the ocean, including the east coast of the United States. The total energy resources in gas hydrates on Earth are estimated to be greater than those of all other known fossil fuels combined — ever.

Large parts of Earth have been examined for the presence of oil and gas fields. Most hydrocarbon regions have been found: those are the known oil and gas regions, including our own North Sea. Within these areas, reservoirs are still being found, but the really big ones are known, and it is becoming increasingly difficult and costly to develop the new ones.

The table below gives an overview of the current proven reserves. There is considerable uncertainty in these numbers, though, both of a technical estimating the size of a reservoir is very difficult and of a political nature countries and companies can have all sorts of reasons to make the reserves look larger or smaller.

According to this table, at the current consumption level we would still have 93 years ahead of us if we were to use all fossil energy. That sounds more reassuring than it is, for several reasons:.

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John huber base hit investing basics While researchers today are working on the development of clean, renewable fuels, our society is still almost entirely dependent on fossil fuels. I highly recommend this course. Multi-product pipelines are used to transport two or more different products in sequence in the same pipeline. Review The technology may be dinosaurial, but fossil-fuel burning continues to be an integral and increasingly costly part of our modern way of living, not least because of the rapid industrialisation of the most populous nations on Earth. Your electronic Certificate will be added to your Accomplishments page - from there, you can solids liquids gas basics of investing your Certificate or add it to your LinkedIn profile. Some sediments were porous such as sand or the skeletons of calcareous animalsothers impermeable such as clay.
Index fund investing bogle Methane, of bacterial or fossil origin, which is released at the bottom of the sea, can form what are known as gas hydrates. One thing is clear: all the oil or gas that has been pumped out is gone forever. Gibb's Phase Rule 4m. It teaches you patience and equally to work hard. The course may offer 'Full Course, No Certificate' instead. Within these areas, reservoirs are still being found, but the really big ones are known, and it is becoming increasingly difficult and costly to develop the new ones. Learn Anywhere.
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Basis for Comparison Solid Liquid Gas Meaning Solid refers to a form of matter which has structural rigidity and has a firm shape which cannot be changed easily. Liquid is a substance, that flows freely, having a definite volume but no permanent shape. Gas refers to a state of matter, do not have any shape but conform to the shape of the container, completely, in which it is put in. Shape and Volume Fixed shape and volume. No fixed shape but has volume. Neither definite shape nor volume.

Random and little sparsely arranged. Random and more sparsely arranged. Fluidity Cannot flow Flows from higher to lower level. Flows in all directions. Molecular motion Negligible molecular motion Brownian molecular motion Free, constant and random molecular motion. Cannot be stored without container. Needs closed container for storage. The particles of a solid are tightly bound and well-arranged in a regular pattern, which does not allow the particles to move freely from one place to another.

The particles continuously vibrate and twist, but there is no motion, as they are too close to each other. As the intermolecular attraction is maximum in solids, and because their shape is fixed, and the particles stay, where they are set. In addition to this, the compression of solid is very tough, as the spaces between molecules are already very less.

A free flowing substance of constant volume having consistency is called as the liquid. It is a type of matter which do not have its shape but takes the shape of the vessel, in which it is held. It contains small particles, which are held tightly by intermolecular bonds. One of the unique property of liquid is surface tension, a phenomenon which makes the fluid possess the minimum surface area. The compression of liquid is a nearly difficult, due to less gap between particles. The particles are closely bound, but not as tightly as in the case of solid.

Thus allowing the particles to move around and mix with one another. Gas is described as a state of matter which diffuses freely in all directions and fills the entire space available, regardless of the quantity. It is made up of particle that does not have a certain shape and volume. The particles can be individual atoms or elemental molecules or compound molecules. In gases, the molecules are loosely held, and so there is a lot of space between molecules to move freely and constantly.

Due to this characteristic, the gas has the ability to fill any container, as well as it can be easily compressed. The matter changes its state from one form to another, when heated or cooled, which is covered under the physical change. So, given below are some processes through which the state of matter can be changed:. Hence, in this article we have learnt that matter is present in three states, i. Solid, liquid and gas. Further, the state of matter are interchangeable, i.

Your email address will not be published. This should make sense because the pressure decreases, so pressure and volume are inversely related. If a sample of gas has an initial pressure of 3. It does not matter which quantity is converted to a different unit; the only thing that matters is that the conversion and subsequent algebra are performed properly.

The following example illustrates this process. Does the answer make sense? This example is similar to Example 5, except now the final pressure is expressed in torr. For the math to work out properly, one of the pressure values must be converted to the other unit.

Let us change the initial pressure to torr:. Torr cancels algebraically from both sides of the equation, leaving. Now we divide both sides of the equation by 1, to isolate V f on one side. Solving for the final volume,. Because the pressure increases, it makes sense that the volume decreases.

If a sample of gas has an initial pressure of torr and an initial volume of 7. Assume that amount and the temperature of the gas remain constant. Breathing certainly is a major contribution to your health! Without breathing, we could not survive.

The lungs are a series of ever-narrowing tubes that end in a myriad of tiny sacs called alveoli. It is in the alveoli that oxygen from the air transfers to the bloodstream and carbon dioxide from the bloodstream transfers to the lungs for exhalation.

The pressure change is caused by the diaphragm, a muscle that covers the bottom of the lungs. When the diaphragm moves down, it expands the size of our lungs. When this happens, the air pressure inside our lungs decreases slightly. This causes new air to rush in, and we inhale. The pressure decrease is slight—only 3 torr, or about 0. We inhale only 0. Exhaling air requires that we relax the diaphragm, which pushes against the lungs and slightly decreases the volume of the lungs.

This slightly increases the pressure of the air in the lungs, and air is forced out; we exhale. Only 1—2 torr of extra pressure is needed to exhale. Another simple gas law relates the volume of a gas to its temperature.

Experiments indicate that as the temperature of a gas sample is increased, its volume increases as long as the pressure and the amount of gas remain constant. The way to write this mathematically is. At this point, the concept of temperature must be clarified. Although the Kelvin scale is the preferred temperature scale, the Celsius scale is also a common temperature scale used in science. The Celsius scale is based on the melting and boiling points of water and is actually the common temperature scale used by most countries around the world except for the United States, which still uses the Fahrenheit scale.

The value of a Celsius temperature is directly related to its Kelvin value by a simple expression:. Thus, it is easy to convert from one temperature scale to another. The Kelvin scale is sometimes referred to as the absolute scale because the zero point on the Kelvin scale is at absolute zero, the coldest possible temperature.

The expression relating a gas volume to its temperature begs the following question: to which temperature scale is the volume of a gas related? The answer is that gas volumes are directly related to the Kelvin temperature. Therefore, the temperature of a gas sample should always be expressed in or converted to a Kelvin temperature.

What happens to the volume of a gas if its temperature is decreased? Assume that all other conditions remain constant. If the temperature of a gas sample is decreased, the volume decreases as well. What happens to the temperature of a gas if its volume is increased? The restriction on its use is that the pressure of the gas and the amount of gas must remain constant. Assume that the pressure and the amount of the gas remain constant.

Multiplying the K to the other side of the equation, we see that our temperature units will cancel:. So, as the temperature is increased, the volume increases. This makes sense because volume is directly proportional to the absolute temperature as long as the pressure and the amount of the remain constant. Other gas laws can be constructed, but we will focus on only two more. The combined gas law The gas law that relates pressure, volume, and absolute temperature.

To apply this gas law, the amount of gas should remain constant. As with the other gas laws, the temperature must be expressed in kelvins, and the units on the similar quantities should be the same. Because of the dependence on three quantities at the same time, it is difficult to tell in advance what will happen to one property of a gas sample as two other properties change.

The best way to know is to work it out mathematically. Using the combined gas law, substitute for five of the quantities:. We algebraically rearrange this expression to isolate V f on one side of the equation:.

The balloon has a volume of 1, mL. What is the new volume of the balloon? The first task is to convert all quantities to the proper and consistent units. The temperatures must be expressed in kelvins, and the pressure units are different so one of the quantities must be converted.

Let us convert the atmospheres to torr:. Now we can substitute the quantities into the combined has law:. To solve for V f , we multiply the K in the denominator of the right side into the numerator on the left, and we divide torr in the numerator of the right side into the denominator on the left:. Notice that torr and kelvins cancel, as they are found in both the numerator and denominator.

The only unit that remains is milliliters, which is a unit of volume. The overall change is that the volume of the balloon has increased by mL. A balloon used to lift weather instruments into the atmosphere contains gas having a volume of 1, L on the ground, where the pressure is 0. Aloft, this gas has a pressure of 6.

What is the new volume of the gas? So far, the gas laws we have used have focused on changing one or more properties of the gas, such as its volume, pressure, or temperature. There is one gas law that relates all the independent properties of a gas under any particular condition, rather than a change in conditions.

This gas law is called the ideal gas law The gas law that relates volume, pressure, temperature, and amount of a gas. The formula of this law is as follows:. In this equation, P is pressure, V is volume, n is amount of moles, and T is temperature. R is called the ideal gas law constant The constant the appears in the ideal gas law.

The variables in this equation do not have the subscripts i and f to indicate an initial condition and a final condition. The ideal gas law relates the four independent properties of a gas under any conditions. The value of R depends on what units are used to express the other quantities.

If volume is expressed in liters and pressure in atmospheres, then the proper value of R is as follows:. This may seem like a strange unit, but that is what is required for the units to work out algebraically. What is the volume in liters of 1. On the right side, the moles and kelvins cancel. Also, because atmospheres appear in the numerator on both sides of the equation, they also cancel. The only remaining unit is liters, a unit of volume.

Dividing both sides of the equation by 3. Note that the conditions of the gas are not changing. Rather, the ideal gas law allows us to determine what the fourth property of a gas here, volume must be if three other properties here, amount, pressure, and temperature are known. What is the pressure of a sample of CO 2 gas if 0.

Under these conditions, 1 mol of any gas has about the same volume. We can use the ideal gas law to determine the volume of 1 mol of gas at STP:. This volume is Because this volume is independent of the identity of a gas, the idea that 1 mol of gas has a volume of Cyclopropane C 3 H 6 is a gas that formerly was used as an anesthetic. How many moles of gas are there in a We can set up a simple, one-step conversion that relates moles and liters:.

Because of its flammability, cyclopropane is no longer used as an anesthetic gas. Freon is a trade name for a series of fluorine- and chlorine-containing gases that formerly were used in refrigeration systems. What volume does 8. Many gases known as Freon are no longer used because their presence in the atmosphere destroys the ozone layer, which protects us from ultraviolet light from the sun. Certain diseases—such as emphysema, lung cancer, and severe asthma—primarily affect the lungs.

Respiratory therapists help patients with breathing-related problems. They can evaluate, help diagnose, and treat breathing disorders and even help provide emergency assistance in acute illness where breathing is compromised.

Therapists must also pass state or national certification exams. Therapists work with equipment such as oxygen tanks and respirators, may sometimes dispense medication to aid in breathing, perform tests, and educate patients in breathing exercises and other therapy. Because respiratory therapists work directly with patients, the ability to work well with others is a must for this career.

It is an important job because it deals with one of the most crucial functions of the body. What makes the ideal gas law different from the other gas laws? Gas laws relate four properties: pressure, volume, temperature, and number of moles. The ideal gas law does not require that the properties of a gas change. Why or why not? A sample of nitrogen gas is confined to a balloon that has a volume of 1.

What will be the volume of the balloon if the pressure is changed to 0. Assume that the temperature and the amount of the gas remain constant. A sample of helium gas in a piston has a volume of What will be the volume of the helium if the pressure on the piston is increased to 1, torr? If a gas has an initial pressure of 24, Pa and an initial volume of mL, what is the final volume if the pressure of the gas is changed to torr?

A gas sample has an initial volume of 0. What would the final pressure of the gas be if the volume is changed to A person draws a normal breath of about 1. Assume that the pressure and amount of the gas remain constant. If pressure and amount are held constant, what is the final volume of the gas in cubic centimeters? What is T f in degrees Celsius and kelvins?

Assuming the amount remains the same, what must be the final volume of a gas that has an initial volume of mL, an initial pressure of torr, an initial temperature of When the nozzle of a spray can is depressed, 0. If the initial temperature of the gas is Use the ideal gas law to show that 1 mol of a gas at STP has a volume of about How many moles of gas are there in a 0.

What is the temperature of the carbon dioxide in kelvins and degrees Celsius? What is the pressure of 0. What is the pressure of 1. To ensure that you understand the material in this chapter, you should review the meanings of the following bold terms in the following summary and ask yourself how they relate to the topics in the chapter. A phase is a certain form of matter that has the same physical properties throughout.

Three phases are common: the solid, the liquid, and the gas phase. What determines the phase of a substance? Generally, the strength of the intermolecular interactions determines whether a substance is a solid, liquid, or gas under any particular conditions. Covalent network bonding is a very strong form of intermolecular interaction. Diamond is one example of a substance that has this intermolecular interaction.

Ionic interactions , the forces of attraction due to oppositely charged ions, are also relatively strong. Covalent bonds are another type of interaction within molecules, but if the bonds are polar covalent bonds , then the unequal sharing of electrons can cause charge imbalances within molecules that cause interactions between molecules.

These molecules are described as polar , and these interactions are called dipole-dipole interactions. A certain rather strong type of dipole-dipole interaction, involving a hydrogen atom, is called hydrogen bonding. On the other hand, equal sharing of electrons forms nonpolar covalent bonds , and the interactions between different molecules is less because the molecules are nonpolar.

All substances have very weak dispersion forces also called London forces caused by the movement of electrons within the bonds themselves. In the solid phase, intermolecular interactions are so strong that they hold the individual atoms or molecules in place.

In many solids, the regular three-dimensional arrangement of particles makes a crystal. In other solids, the irregular arrangement of particles makes an amorphous solid. In liquids, the intermolecular interactions are strong enough to keep the particles of substance together but not in place. Thus, the particles are free to move over each other but still remain in contact. In gases, the intermolecular interactions are weak enough that the individual particles are separated from each other in space.

The kinetic theory of gases is a collection of statements that describe the fundamental behavior of all gases. Among other properties, gases exert a pressure on their container. Pressure is measured using units like pascal , bar , atmosphere , or mmHg also called a torr. There are several simple relationships between the variables used to describe a quantity of gas. These relationships are called gas laws.

The combined gas law relates the volume, pressure, and absolute temperature of a gas sample. All of these gas laws allow us to understand the changing conditions of a gas. The ideal gas law relates the pressure, volume, amount, and absolute temperature of a gas under any conditions. These four variables are related to the ideal gas law constant , which is the proportionality constant used to calculate the conditions of a gas.

Because the conditions of a gas can change, a set of benchmark conditions called standard temperature and pressure STP is defined. How many grams of oxygen gas are needed to fill a A breath of air is about 1. If the pressure is 1. Use an average molar mass of The balanced chemical equation for the combustion of propane is as follows:.

The equation for the formation of ammonia gas NH 3 is as follows:. By what factor has the water expanded in going from the liquid phase to the gas phase? Predict whether NaCl or NaI will have the higher melting point. Hint: consider the relative strengths of the intermolecular interactions of the two compounds. A standard automobile tire has a volume of about 3. Tires are typically inflated to an absolute pressure of Using this information with the ideal gas law, determine the number of moles of air needed to fill a tire if the air temperature is If an automobile tire see Exercise 9 is inflated to Assume that the volume and the amount of the gas remain constant.

NaCl; with smaller anions, NaCl likely experiences stronger ionic bonding. Previous Chapter. Table of Contents. Next Chapter. Identify the types of interactions between molecules. Note For many substances, there are different arrangements the particles can take in the solid phase, depending on temperature and pressure.

The boiling point of a substance is the temperature that separates a liquid and a gas. Example 1 What intermolecular forces besides dispersion forces, if any, exist in each substance? Because ionic interactions are strong, it might be expected that potassium chloride is a solid at room temperature. Ethanol has a hydrogen atom attached to an oxygen atom, so it would experience hydrogen bonding. If the hydrogen bonding is strong enough, ethanol might be a solid at room temperature, but it is difficult to know for certain.

Ethanol is actually a liquid at room temperature. Elemental bromine has two bromine atoms covalently bonded to each other. Because the atoms on either side of the covalent bond are the same, the electrons in the covalent bond are shared equally, and the bond is a nonpolar covalent bond.

Thus, diatomic bromine does not have any intermolecular forces other than dispersion forces. It is unlikely to be a solid at room temperature unless the dispersion forces are strong enough. Bromine is a liquid at room temperature. Skill-Building Exercise What intermolecular forces besides dispersion forces, if any, exist in each substance?

Concept Review Exercise What types of intermolecular interactions can exist in compounds? Answer polar and nonpolar covalent bonding, ionic bonding, dispersion forces, dipole-dipole interactions, and hydrogen bonding. Key Takeaways A phase is a form of matter that has the same physical properties throughout.

Molecules interact with each other through various forces: ionic and covalent bonds, dipole-dipole interactions, hydrogen bonding, and dispersion forces. Exercises List the three common phases in the order you are likely to find them—from lowest temperature to highest temperature. Answers solid, liquid, and gas. Solids In the solid state, the individual particles of a substance are in fixed positions with respect to each other because there is not enough thermal energy to overcome the intermolecular interactions between the particles.

Liquids If the particles of a substance have enough energy to partially overcome intermolecular interactions, then the particles can move about each other while remaining in contact. Gases If the particles of a substance have enough energy to completely overcome intermolecular interactions, then the particles can separate from each other and move about randomly in space. Example 2 What state or states of matter does each statement, describe? This state has a definite volume. This state has no definite shape.

This state allows the individual particles to move about while remaining in contact. Solution This statement describes either the liquid state or the solid state. This statement describes either the liquid state or the gas state. This statement describes the liquid state.

Skill-Building Exercise What state or states of matter does each statement describe? This state has a definite shape. Concept Review Exercise How do the strengths of intermolecular interactions in solids and liquids differ? Answer Solids have stronger intermolecular interactions than liquids do.

Looking Closer: Water, the Most Important Liquid Earth is the only known body in our solar system that has liquid water existing freely on its surface. Key Takeaway Solids and liquids are phases that have their own unique properties. Exercises What are the general properties of solids? What are the general properties of liquids.

What are the general properties of gases? Answers hard, specific volume and shape, high density, cannot be compressed. Example 3 Write a conversion factor to determine how many atmospheres are in 1, mmHg. Solution Because 1 mmHg equals 1 torr, the given pressure is also equal to 1, torr.

Skill-Building Exercise Write a conversion factor to determine how many millimeters of mercury are in 9. Concept Review Exercise What is pressure, and what units do we use to express it? Answer Pressure is the force per unit area; its units can be pascals, torr, millimeters of mercury, or atmospheres. Key Takeaway The gas phase has certain general properties characteristic of that phase. Exercises What is the kinetic theory of gases? Why does a gas exert pressure? How many torr are there in 1.

Convert torr into pascals. Answers Gases are composed of tiny particles that are separated by large distances. Example 4 What happens to the volume of a gas if its pressure is increased? Solution If the pressure of a gas is increased, the volume decreases in response. Skill-Building Exercise What happens to the pressure of a gas if its volume is increased? Example 5 If a sample of gas has an initial pressure of 1.

Solution The key in problems like this is to be able to identify which quantities represent which variables from the relevant equation. Skill-Building Exercise If a sample of gas has an initial pressure of 3. Example 6 If a sample of gas has an initial pressure of 1. Solution This example is similar to Example 5, except now the final pressure is expressed in torr.

Let us change the initial pressure to torr: 1. Skill-Building Exercise If a sample of gas has an initial pressure of torr and an initial volume of 7. To Your Health: Breathing Breathing certainly is a major contribution to your health!

Note The Kelvin scale is sometimes referred to as the absolute scale because the zero point on the Kelvin scale is at absolute zero, the coldest possible temperature. Example 7 What happens to the volume of a gas if its temperature is decreased?

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States of Matter : Solid Liquid Gas

It is also a liquid metaphor to refer to flujos de capital, which relates to the transfer of foreign investment or loans into a nation's economy. A standard. States of Matter - The matter is classified into solids, liquids, and gases in termed physical classification of matter. Solid, liquids and gas are the. Solids that change to gas pass through the liquid state first. However, sometimes solids change directly to gases and skip the liquid state. The.