Chemistry

Partition coefficient (Kx) was determined from the following equation, according to the pseudo-phase model [23, 24]:

The three gas laws that were covered during this experiment were: Boyle's law, Charles' law, and Gay-Lussac's law. These laws support this experiment's findings by showing the increased and decreased values. Boyle is an indirect (1/α), and Charles and Gay-Lussac are both a direct (α) relationship.

In most circumstances, substances exist as three states of matter which are denoted to as phases: a solid, a liquid, or a gas.1 Those phases change from one to the other through pressure and temperature. The shape and volume define each phase. A solid has uniform shape and volume, a liquid has uniform volume but diverse shape, and a gas has various shapes and volumes.1 No matter what container the gas is in, a force, referred to as pressure, is exerted by the gas on the walls of the container to evenly fill out the container. The pressure is dependent on three variables which are container’s volume, gas’s volume in the container, and gas’s temperature in the container. Those variables can be explained in the Ideal Gas Law, PV=nRT.2 This

Boyle's Law was named after its maker, Robert Boyle. He began to study how to compress gases in 1660, and in all of his experiments he said, "At a fixed temperature, the volume of a gas is inversely proportional to the pressure exerted by the gas." In a math equation it would be written pressure times volume equals a constant (PxV=Constant) (Blauch, Gas Laws). The law was named after him in 1662 (ChemTeacher). Following his studies he published a book in 1680. He told about how all gases had different properties like volume, temperature, and pressure that can be observed with senses; the value of these properties can determine what state the gas being tested

where p is the density, g is the acceleration due to gravity, h is the height of the solution and r is the radius of the capillary.

One of the most important things about gases is that, despite wide differences in chemical properties, all the gases more or less obey the gas laws. The gas laws deal with how gases behave with respect to pressure, temperature, volume and amount. This uniformity of physical behavior was of great interest with early scientists. It is one of the dogmas of scientists that the behavior of a material is a reflection of the particles that make up the substance. In other words, differences between solids, liquids and gases reflect the movement of the small particles that compose all matter. This assumption is part of the Kinetic Theory Of Gases (Kinetic is from the Greek word for motion). Historically, the description of the gas properties has been summarized by the mathematical equations describing the relationships between the gas volume, pressure and temperature. These equations, named after the scientist who first demonstrated their validity, have been labeled the gas laws. These gas laws are best understood within the framework described as the kinetic theory of gases:

(b) When d = 1.0 10-3 mm, d-1/2 = 31.6 mm-1/2, and, using Equation 8.7,

with: S: Seebeck coefficient, σ: Electrical conductivity, T : Absolute temperature, S2σ: Power factor andκ : Thermal conductivity.

In other lessons, we learned about different gas laws: Boyle’s Law, Charles’ Law and Gay-Lussac’s Law. What happens if we combine all these laws together? We come up with a whole new gas law: The Combined Gas Law. This will be our lesson’s focus.

We want to try and develop a material balance equation that tries to give an accurate estimate of the original gas in place in a coalbed methane reservoir considering the absorbed gases, free gases, rock compressibility and certain factors that have strong effect on the original gas in place.

Bear in mind what G. E. Archie said about his equations. "It should be remembered that the equations given are not precise and represent only approximate relationships.

The theory of Corresponding States proposes that all gases will exhibit the same behaviour, e.g. z-factor, when viewed in terms of reduced pressure, reduced volume, and reduced temperature.

Therefore, we will try to fit it with the general form of this function, shown below:

UNIT – VI Mixtures of perfect Gases – Mole Fraction, Mass friction Gravimetric and volumetric Analysis – Dalton’s Law of partial pressure, Avogadro’s Laws of additive volumes – Mole fraction , Volume fraction and partial pressure, Equivalent Gas const. And Molecular Internal Energy, Enthalpy, sp. Heats and Entropy of Mixture of perfect Gases and Vapour, Atmospheric air - Psychrometric Properties – Dry bulb Temperature, Wet Bulb Temperature, Dew point Temperature, Thermodynamic Wet Bulb Temperature, Specific Humidity, Relative Humidity, saturated Air, Vapour pressure, Degree of saturation – Adiabatic Saturation , Carrier’s Equation – Psychrometric chart. UNIT - VII Power Cycles : Otto, Diesel, Dual Combustion cycles, Sterling Cycle, Atkinson Cycle, Ericcson Cycle, Lenoir Cycle – Description and representation on P–V and T-S diagram, Thermal Efficiency, Mean Effective Pressures on Air standard basis – comparison of Cycles. 4

Chapter 1 Topics  Matter and its Classification  Physical and Chemical Changes and Properties of Matter  Energy and Energy Changes (skip)  Scientific Inquiry Chapter 1 Math Toolboxes  Scientific Notation (exponential notation)  Significant Figures  Units and Conversions