CH 104 Lecture Notes - Lecture 1: Strong Interaction, Gas Laws, Gas Constant

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carminehound79

25 Oct 2016

School

University of Alabama

Department

Chemistry

Course

CH 104

Professor

Monica Vasiliu

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Document Summary

Solid: molecules locked in place, definite shape and volume, high density, slow particle movement, very strong interaction between particles. Liquid: molecules have enough kinetic energy to overcome some of the attractive forces, molecules have limited movement, high density, fixed volume but takes the shape of its container, strong interaction between particles. Gas: molecules have complete freedom of motion, kinetic energy overcomes the attractive forces, expands to fill its container, low density, zero interaction between particles, fast particle movement. Kinetic energy of gas particles increases with increasing temperature. When particles collide, they rebound and travel in new directions. When gas particles collide with a container it creates a pressure. Boyle"s la(cid:449) relates to the pressure a(cid:374)d (cid:448)olu(cid:373)e of a gas: pressure and volume are inversely related, pressure x volume = constant, p1v1=p2v2. Charles"s la(cid:449) relates the (cid:448)olu(cid:373)e of a gas to its kel(cid:448)i(cid:374) te(cid:373)perature: volume/temperature =constant, volume of the gas is proportional to its kelvin temperature, v1/t1 = v2/t2.

Related Questions

To understand the kinetic molecular descriptions of solids, liquids, and gases.

The following table gives information about the behavior of molecules in solids, liquids, and gases.

	Solid	Liquid	Gas
Density	high	high	low
Molecular movement (with respect to one another)	minimally	slow	fast
Compressibility and thermal expansion	fixed volume	fixed volume	variable volume
Do they expand to fill their container?	no	no	yes
Do they take the shape of their container?	no	yes	yes

Part B

Consider equal volumes (say 1 L) of a given substance in the solid, liquid, and gas phases. Arrange them in order of decreasing mass based on the trend for the average substance. If the mass difference between samples is relatively small (10%or less), rank the items as equivalent.

Rank from greatest to least mass. To rank items as equivalent, overlap them.

1L of substance in the solid phase, 1L of substance in the liquid phase, 1L of substance in the gas phase

Greatest Mass Least Mass

Part C

Match each description to the appropriate phase of matter.

A substance with a fixed volume and fixed shape

A substance with no fixed volume or shape

A substance with a fixed volume and no fixed shape

Solid Liquid Gas

M 121 1 201 Ideal Gas Law (PV n Experiment to T ) Determine the Ideal Gas Constant R 1. Conduct basic measurements, measurement , mathematical calculations and conversions for of volume, pressure, and temperature: calculate percent error and account for sources of error in an e xperimental result name and by following safety proced ty experiments for a redox reaction by using equipment identifiable by form chemical calculations using mass, mole and volumes and idenify limitatios of measuring devices in order to state the uncertainty/significant figures in measurements and calculation results. 5. Demonstrate a proficiency in relating the chemistry of gases to everyday phenomenon. Introduction Molecules in gases have very little attraction for one another, because relative to their size, they are so far apart from each other. For this reason we can often assume that a gas behaves "idcally." meaning that the physical behavior of the gas is independent of the composition of the gas. If a gas behaves ideally, then its physical properties can be described by the Ideal Gas Equation: Let's consider why the variables in the ideal gas equation have the relationships expressed in Equation 1aã The ideal gas equation assumes that there are no attractive forces between gas molecules. One can picture two billiard balls bouncing off one another in a totally clastic collision. If these molecules are placed in a balloon the collisions will occur not only with each other but also with the wall of the balloon, causing the balloon to expand. This expansion can be measured as a volume (V). More molecules will cause more collisions and thus more expansion. Therefore the quantity of molecules or number of moles (n) is directly proportional to the volume, and thus volume and number of moles appear on opposite sides of the equation. Another factor to consider is the kinetic energy of these molecules. Kinetic energy is related to the temperature (T) of the molecules, in that the kinetic energy. If the collisions with the wall of the balloon are happening at a very high speed due to high kinetic energy, the collisions will be harder and more frequent and thus the wall of the balloon will be pushed out further (a larger volume) than if the kinetic energy were less. The result is that volume is also directly proportional to the temperature. This relationship is seen in Equation la with (T) on the right side of the equation and (V) on the left. higher the temperature the greater the considered. While the molecules inside the balloon are pushing the balloon out, there are also molecules in thea Finally the pressure of the outside environment (atmospheric pressure) needs to be 59

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CH 104 Lecture Notes - Lecture 1: Strong Interaction, Gas Laws, Gas Constant

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