Gas+Laws+and+Kinetics

http://www.youtube.com/watch?v=28F_oPDZHSk States the volume of a definite quantity of dry gas is inversely proportional to the pressure, provided the temperature remains constant. Mathematically Boyle's law can be expressed as P1V1 = P2V2
 * media type="youtube" key="vPWFjmX-1aI?fs=1" height="385" width="480"Boyle's Law** -
 * V1 is the original volume
 * V2 is the new volume
 * P1 is original pressure
 * P2 is the new pressure

Suppose you have a gas with 45.0 ml of volume and has a pressure of 760.mm. If the pressure is increased to 800mm and the temperature remains constant then according to Boyle's Law the new volume is 42.8 ml. (760mm)(45.0ml) = (800mm)(V2) V2=42.8ml

[|Boyle's Experiment]s

Definition terms Catalyst- a substance that increases the rate of a chemical reaction by lowering activation energies but is not itself consumed in the reaction.

Activation energy- the minimum amount of energy required by reacting particles in order to form the activated complex and lead to a reaction. Ideal gas- the physical behavior of ideal gas in terms of the temperature, volume, and pressure, and number of moles of a gas that are presented. Kinetic molecular- explains the properties of gases in terms of energy, size, and motion of their particles. [|Kinetic Theory]

Absolute zero- The theoretical temperature at which molecules of any substance have the least energy,all the molecular motion ceases, and a perfect gas.

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Avogadro's principle- The principle that equal volumes of all gases under identical conditions of pressure and temperature contain the same number of molecules.



Avogadro's my name and I'm a gas! Some said my theory just wouldn't last! It's not hard. It's safe to assume, that the same number particles occupy the same volume! I wrote the mole, the unit, And it seems like on every test we always use it! I am not here to cause no trouble I am just here to do the Super Mole shuffle!

OR, in other words: Equal volumes of gas at the same temperature and pressure will contain the same number of gas particles.

Source: “Glencoe Science Chemistry Matter and change” Kelvin- the SI base unit of temperature. Entropy- a measure of the disorder of randomness of the particles of a system.( change in heat) Enthalpy- the heat content of a system at constant preassure.



Molar Volume- The volume occupied by one mole of a substance int he form of a solid, liquid, or gas. STP-STP or Standard Temperature and Pressure, corresponds to 273 K (0 degrees Celsius) and 1 atm pressure. STP is often used for measuring gas density and volume.



Entropy:

Entropy is the quantitative measure of disorder in a system. The concept comes out of

[|thermodynamics], which deals with the transfer of [|heat energy] within a system.

Collision Theory: Theory of chemical reaction proposing that the rate of product formation is equal to the number of reactant-molecule collisions multiplied by a factor that corrects for low-energy-level collisions.

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[]

Spontaneity : The quality or state of being spontaneous, or acting from native feeling, proneness, or temperament, without constraint or external force. The relationship expressed by Boyle's Law, Charles’ Law, Avogadro’s Principle, and Dalton’s Law:

=LAWS:=

Dalton’s law of partial pressures – States that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases in the mixture Charles Law: Charles's Law, or the law of volumes, was found in 1787. It says that, for an ideal gas at constant pressure, the volume is proportional to the temperature.States that the volume of a given mass of gas is directly proportional to its Kelvin temperature at constant

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Boyle's Law: States that the volume of a given amount of gas held at a constant temperature varies inversely with the pressure Boyle's Law shows that, at constant temperature, the product of an [|ideal gas's] pressure and volume is always constant. It was published in 1622. It can be determined experimentally using a pressure gauge and a variable volume container. It can also be found through the use of logic; if a container, with a fixed amount of molecules inside, is reduced in volume, more molecules will hit the sides of the container per unit time, causing a greater pressure. As a mathematical equation, Boyle's law is:



The [|state] of an amount of [|gas] is determined by its pressure, volume, and temperature. The modern form of the equation is: Where P is the pressure (Pa), V the volume (dm3) of a gas, and k1 (measured in [|joules]) is the constant from this equation. for virtual lab go here[|Boyle's law]



=POTENTIAL ENERGY☺=

KINETICS

media type="youtube" key="UNn_trajMFo?fs=1" height="385" width="480" media type="youtube" key="Rn470XtSYK0" width="425" height="350" Kinetics is the study of the rate of chemical reactions, such as the acid dehydration of sugar, shown in this photograph.



Question #2

Boyle’s Law: P1V1 = P2V2 Charles’ Law: V1/T1 = V2/T2

Avogadro’s Principle: When measured at the same Kelvin temperate and pressure, equal volumes of gases contain equal numbers of mole. At standard, temperature, and pressure one mole of gas occupies 22.4 liters of volume. Dalton’s Law: The total pressure of a mixture of nonreacting gases is the sum of their individual partial pressures PT = P1 + P2 + … + Pn Boyle’s Law and Charles’ Law can be related through the Combined Gas Law which says that (T must be in Kelvin). In some situations Dalton’s Law can be used to find the pressure that is plugged into the equation, and Avogadro’s Principle can be used to find the volume.

Boyle’s Law The effects of pressure are more easily observed with gases than with any other element. The Englishman, Robert Boyle, formulated a law on the compressibility of gases, which establishes a relationship between the volume occupied by a gas and the pressure to which it is exposed. Boyle’s Law states that the volume of a gas is inversely proportional to its pressure. Question # 3

Particle size The particle size of a [|spherical] object can be unambiguously and quantitatively defined by its [|diameter]. However, a typical material object is likely to be irregular in [|shape] and non-spherical. The above quantitative definition of particle size cannot be applied to non-spherical particles. There are several ways of extending the above quantitative definition, so that a definition is obtained that also applies to non-spherical particles. Existing definitions are based on replacing a given particle with an imaginary [|sphere] that has one of the properties identical with the particle.
 * Volume based particle size equals the diameter of the sphere that has same volume as a given particle.
 * Weight based particle size equals the diameter of the sphere that has same weight as a given particle.
 * Area based particle size equals the diameter of the sphere that has the same [|surface] area as a given particle.
 * [|Hydrodynamic] or [|aerodynamic] particle size equals the diameter of the sphere that has the same [|drag] coefficient as a given particle

Particle motion

Question #9 Activation Energy- The least amount of energy needed for a chemical reaction to take place. Some elements and compounds react together naturally just by being close to each other, and their activation energy is zero. Others will react together only after a certain amount of energy is added to them. Striking a match on the side of a matchbox, for example, provides the activation energy (in the form of heat produced by friction) necessary for the chemicals in the match to ignite. Activation energy is usually expressed in terms of joules per mole of reactants. Catalyst effects activation energy, because catalyst varies the path of reaction or you can say mechanism of reaction due to which activation energy gets lower as a result of which fruitful collisions took place at relatively lower temperature so more chances for molecules to cross activation complex.
 * 1) 5. Interpret graphs of gas law data to determine relationships.

The Gas Laws

These gas laws led to several important concepts in Physics. Boyles Law: Pressure is inversely proportional to the volume:

We can plot the data as a graph: We can see that the data fit into a pattern called a hyperbola. If, however we plot pressure against 1/volume we get a linear (straight line) graph.

Since the line goes through the origin, we say that the two quantities are directly proportional.
 * So we can say that
 * 1 /Volume (m-3) ||


 * Pressure (kPa) ||

P µ 1/V

P = k/V where k is a constant.
 * Therefore:

PV = constant.6. Calculate partial pressures of a gaseous mixture using Dalton's Law?The total pressure of a mixture of gases equals the sum of the pressures that each would exert if it were present alone."
 * Rearranging:

Ptotal = P1 + P2 +. . . Pn

is the total pressure of a sample which contains a mixture of gases
 * Pt

, etc. are the partial pressures (in the same units) of the gases in the mixture Pdry gas = Ptotal - Pwater vapor
 * P1, P2, P3

This means we must get the water vapor pressure from somewhere.

We get it from a table because the water vapor pressure depends only on the temperature, NOT how big the container is or the pressure of the other gas.


 * Temp (oC) || Vapor Pressure (mmHg) || Temp (oC) || Vapor Pressure (mmHg) || [[image:http://www.kentchemistry.com/images/links/gases/satvap.gif]] ||


 * -10 || 2.15 || 40 || 55.3 ||  ||

Question #10Entropy:The measure of the disorder of a system, usually denoted by the letter S. A highly ordered system has low entropy. Ex. A block of ice will increase in Entropy as it melts. Since spontaneity is a process that will occur without any energy input from the surroundings, it is a process that will occur on its own. I think entropy effects spontaneity because it will ether make the process of spontaneity go faster or go slower. So entropy will ether increase the time of spontaneity or decrease it. Question #1Absolute Zero- Absolute zero is the point where no more heat can be removed from a system, according to the absolute or thermodynamic temperature scale. This corresponds to 0 K or -273.15°C. In classical kinetic theory, there should be no movement of individual molecules at absolute zero, but experimental evidences shows this isn't the case.
 * 0 || 4.58 || 60 || 149.4 ||  ||
 * 5 || 6.54 || 80 || 355.1 ||^  ||
 * 10 || 9.21 || 95 || 634 ||^  ||
 * 11 || 9.84 || 96 || 658 ||^  ||
 * 12 || 10.52 || 97 || 682 ||^  ||
 * 13 || 11.23 || 98 || 707 ||^  ||
 * 14 || 11.99 || 99 || 733 ||^  ||
 * 15 || 12.79 || 100 || 760 ||^  ||
 * 20 || 17.54 || 101 || 788 ||^  ||
 * 25 || 23.76 || 110 || 1074.6 ||^  ||
 * 30 || 31.8 || 120 || 1489 ||^  ||
 * 37 || 47.07 || 200 || 11659 ||

Kelvin- Kelvin is a temperature scale designed so that zero degrees K is defined as absolute zero (at absolute zero, a hypothetical temperature, all molecular movement stops - all actual temperatures are above absolute zero) and the size of one unit is the same as the size of one degree Celsius. Water freezes at 273.16K; water boils at 373.16K. [ K = C + 273.16°, F = (9/5)C + 32°].

Molar Volume- The volume occupied by one mole of a substance in the form of a solid, liquid, or gas. Also known as molal volume; mole volume.

7THE COMBINED GAS LAW FORMULA

The Combined Gas Law Formula is the relationship of changing pressure, temperature, and volume of an ideal gas. The same amount of the same gas is given at two different sets of conditions. Let's call the first set of measurements, 'condition #1,' and the second set of measurements, 'condition #2.' We could label the pressure, temperature and volume symbols each with the subscripted number of the condition it represents. P1 is the pressure at condition #1. P2 is the pressure at condition #2. V1 is the volume at condition #1, etc. The gas laws apply to both conditions, so P1 V1 =n R T1 and P2 V2= n R T2. R is always the same Universal Gas Constant. If we are considering the same gas only at two different conditions, then n1 = n2. Since they are both equations, we could divide one equation by the other to get:

=R= ||  ||   ||   || n1n2 ||   ||   ||   ||   || || = || || or || || = || || or || || = || ||
 * || R
 * P1V1 ||  || n1 R T1 ||   || P1V1 ||   || n1 T1 ||   || P1V1 ||   || T1 ||
 * P1V1 ||  || n1 R T1 ||   || P1V1 ||   || n1 T1 ||   || P1V1 ||   || T1 ||
 * P2V2 ||  || n2 R T2 ||   || P2V2 ||   || n2 T2 ||   || P2V2 ||   || T2 ||

The last form can be a very useful one. This is the form of the Combined Gas Law Formula that Chemtutor finds easiest to remember. The formulas that most books call the Gas Laws are all contained in the Combined Gas Law. The Combined Law Formula is the one to use if you have any doubt about which of the Gas Laws to use.


 * || P

1V1 ||  || T1 || || = || ||
 * P2V2 ||  || T2 ||   ||

KNOW THIS 7. Solve problems using the gas law of Boyle's and Charles'.

1.how many torr are in 0.311 atm.

1atm = 760 mm Hg (or torr), \

(0.311 atm) • (760 torr / 1 atm) = 236 torr

2.how you find 125 psi in mm Hg:

(125 psi) • (1 atm / 14.7 psi) • (760 mm Hg / 1atm) = 6.24 • 10^3 mm Hg

3.the pressure inside a 6.0 L cylinder is filled with enough air to exert 4.0 atm against the inside of the cylinder. Suppose a piston compressed the air from 6.0 L to 2.0 L. How many atms is that?

( 4.0 atm • 6.0 L) = ( ? atm • 2.0 L)

( 4.0 atm • 6.0L ) / 2.0 L = 12 atms

4.A balloon is filled with 2.80 L gas at an unknown temperature. When the balloon is submerged in ice water at

0 °C and the volume shrinks to 2.57 L. What is the missing temperature in Kelvins?

Since 0 °C = 273.15 Kelvins, we can just substitute Kelvins for Celcius since division by zero isn't allowed.

2.80L / ? Kelvins = 2.57L / 273.15 Kelvins

2.80L / ? Kelvins = 0.009409 L / Kelvins

(0.009409 L / Kelvins) / 2.80L = 297 Kelvins

? Kelvins = 297 K

DALTON'S LAW media type="youtube" key="6-U0B4iSCOQ" width="425" height="350"

http://www.youtube.com/watch?v=vFB3u6JL7Qc

Boyle's Law http://www.youtube.com/watch?v=J_I8Y-i4Axc

Charle's Law http://www.youtube.com/watch?v=oIfFoiwRCVE

Avogadro’s Principle http://www.youtube.com/watch?v=13WUqWd_Yk8 []

8. Identify and interpret the components of a potential energy diagram

In a chemical reaction; reactants --> products ΔPE = PE products - PE reactants PE can be thought as heat energy (H) Therefore, ΔH (kJ) = H products - H reactants When ΔH is negative H products < H reactants and the reaction is exothermic. When ΔH is positive H products > H reactants and the reaction is endothermic.

Collision theorymedia type="youtube" key="a6UklfhlWQg?fs=1" height="385" width="480"



9. Define activation energy and explain how a catalyst affects it.

A catalyst is a chemical substance usually used in small amounts relative to the reactants and this compound alters the rate of reaction, thereby increasing it without being consumed in the entire process

Catalysts are also divided into two groups:
 * 1) Homogenous catalysts (like enzymes and aqueous ions that uniformally mixed with the reactants)
 * 2) Heterogeneous catalysts (provide surface for the reaction to occur)

**A few Examples of Catalysts**
==


 * A piece of platinum foil is a catalyst used in the combustion of methane in air.
 * Epoxy ethane is manufactured by reacting ethene in the presence of a Silver catalyst.
 * Benzene reacts with Chlorine or Bromine in the presence of catalyst named Aluminum Chloride (AlCl3) and Aluminum Bromide (AlBr3).
 * The important Friedel-Crafts alkylation of Benzene used Aluminum Chloride (AlCl3) as a catalyst.
 * Enzymes are the examples of metabolic catalyst that speed up the biological process inside the human body like nutrition, respiration.etc.
 * Temperature and Time are also important examples of catalysts.
 * Use of Platinum as catalysts in the hydrogenation of Alkenes is an example of heterogeneous catalyst.

Catalysts plays very important role in a chemical reaction. Due to the presence of these catalysts, we are able to get the desired product as soon as possible. Catalysts do not alter the position of equilibrium; they only change the rate of the reaction. ==

Collision Theory-Collision theory is a theory proposed by Max Traut and William Lewis in 1916 and 1918, that qualitatively explains how chemical reactions occur and why reaction rates differ for different reactions. For a reaction to occur the reactant particles must collide. Only a certain fraction of the total collisions cause chemical change; these are called successful collisions. The successful collisions have sufficient energy (activation energy) at the moment of impact to break the existing bonds and form new bonds, resulting in the products of the reaction. Increasing the concentration of the reactants and raising the temperature bring about more collisions and therefore more successful collisions, increasing the rate of reaction. 

Spontaneity-

The above examples show three important points about spontaneity * Spontaneity depends on temperature: ice melts at 250C, but not below 00C, for example. To determine if a reaction is spontaneous, you must compute the change in the Gibbs free energy for the reaction. ||
 * A reaction is said to be //spontaneous// if it proceeds without any external energy being added. Some basic examples include:
 * Ice melting at 250C: H2O(s) -> H2O(l)
 * Hydrogen burning: 2H2(g) + O2(g) -> 2H2O(g)
 * Spontaneous does not mean "fast": hydrogen and oxygen have a rate constant of ~0 at room temperature, but the reaction is still spontaneous at that temperature
 * The reverse of a spontaneous reaction is not spontaneous: water does not turn into hydrogen and oxygen unless you add energy.



Enthalpy- <span style="border-collapse: separate; font-family: sans-serif,helvetica,sans-serif;">a measure of the total energy of at thermodynamic system. It includes the internal energy, which is the energy required to create a system, and the amount of energy required to make room for it by displacing its environment and establishing its volume and pressure.

<span style="font-family: Helvetica; font-size-adjust: none; font-size: 12px; font-stretch: normal; font-style: normal; font-variant: normal; font-weight: normal; line-height: normal; margin: 0px;">

<span style="border-collapse: collapse; color: #000000; display: block; font-family: 'Times New Roman','Times New Roman'; font-size-adjust: none; font-size: 13px; font-stretch: normal; font-style: normal; font-variant: normal; font-weight: normal; letter-spacing: normal; line-height: 19px; orphans: 2; text-align: left; text-indent: 0px; text-transform: none; white-space: normal; widows: 2; word-spacing: 0px;">10. Define entropy and explain its effect on spontaneity.

<span style="border-collapse: separate; color: #000000; display: block; font-family: Verdana,Arial,sans-serif; font-size-adjust: none; font-size: medium; font-stretch: normal; font-style: normal; font-variant: normal; font-weight: normal; letter-spacing: normal; line-height: normal; orphans: 2; text-align: left; text-indent: 32px; text-transform: none; white-space: normal; widows: 2; word-spacing: 0px;">**Entropy measures the spontaneous dispersal of energy: how //much// energy is spread out in a process, or how //widely// spread out it becomes — at a specific temperature.**

<span style="border-collapse: separate; color: #000000; display: block; font-family: Verdana,Arial,sans-serif; font-size-adjust: none; font-size: medium; font-stretch: normal; font-style: normal; font-variant: normal; font-weight: normal; letter-spacing: normal; line-height: normal; orphans: 2; text-align: left; text-indent: 32px; text-transform: none; white-space: normal; widows: 2; word-spacing: 0px;">**<span style="border-collapse: separate; color: #000000; font-family: Verdana,Arial,sans-serif; font-size-adjust: none; font-size: medium; font-stretch: normal; font-style: normal; font-variant: normal; font-weight: normal; letter-spacing: normal; line-height: normal; orphans: 2; text-indent: 32px; text-transform: none; white-space: normal; widows: 2; word-spacing: 0px;">ntropy change = “energy dispersed”/T, or qreversible/T, as in phase changes like melting or vaporization where ΔS = ΔHfusion /T or ΔHvaporization /T, respectively. ** Potential Energy Diagram:

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