Download presentation

1
DENSITY AND PRESSURE By Anoushka Bhat

2
DENSITY Density is how much something of a set volume weighs. This is generally measured by taking a cubic centimeter of a substance (cm^-3). If we take a cubic centimeter of some commonly known substances, we can see that they weigh different amounts: DENSITY is a physical property of matter, as each element and compound has a unique density associated with it. Density defined in a qualitative manner as the measure of the relative "heaviness" of objects with a constant volume. For example: A rock is obviously more dense than a crumpled piece of paper of the same size. A Styrofoam cup is less dense than a ceramic cup. Density may also refer to how closely "packed" or "crowded" the material appears to be - again refer to the Styrofoam vs. ceramic cup.

3
**Calculating DENSITY Calculating Density**

The best way to calculate the density of any material is to take a cubic centimeter of it and weigh it. That will give you the mass of the substance per cubic centimeter. For lead (Pb), each cubic centimeter of it weighs grams, making its density grams per cubic centimeter, or g / cm^-3 if you're scientifically minded. For lead, 1 cubic centimeter weighs grams, while 2 grams weighs grams and so on; so we see that the ratio of grams per cubic centimeter holds fast. The definition of density functions. The Formula For Density We calculate density by dividing mass by volume as shown to the right. The units can actually be of any kind, as long as they are the same between substances to be compared. We could measure density in milligrams per cubic mile, or kilotons per cubic nanometer, it makes no difference. As long as the units are clearly stated, conversion to standard units is easily achieved. Mass vs. Weight: Although the terms mass and weight are used almost interchangeably, there is a difference between them. Mass is a measure of the quantity of matter, which is constant all over the universe. Weight is proportional to mass but depends on location in the universe. Weight is the force exerted on a body by gravitational attraction (usually by the earth). Example: The mass of a man is constant. However the man may weigh: 150 lbs on earth, 25 lbs on the moon (because the force of gravity on the moon is 1/6 that of the earth), and be "weightless" in space.

4
**Density of a liquid HOW TO FIND THE DENSITY OF A LIQUID?**

Apparatus: 100ml graduated cylinder, triple beam balance, calculator, 2 unknown liquids. Procedure: 1) Find the mass of the empty graduated cylinder. 2) Pour unknown liquid #1 into the graduated cylinder to the 50 ml. level. 3) Find the mass of the graduated cylinder with 50ml of unknown liquid #1. 4) Repeat steps 1-3 for unknown liquid #2. We can calculate density of a liquid using the formula: Density= Mass/Volume where mass is that for just the liquid (you must subtract out the mass of the graduated cylinder).

5
Density of Air To find the density of air the mass of a sample of air is measured and compared to the volume it occupies. A problem with giving a value for the density of air is that there is no set value. The density of air will change with height and with a change in the weather. The density of air is going to depend on the air pressure, the temperature of the air and how much moisture is in the air. The density of air under standard conditions is only milligrams per cubic centimeter under standard conditions. Measuring the density is done by finding the mass of an evacuated glass sphere, letting the air back into the sphere, and finding the new mass. This is done with the sphere on one pan of an equal-arm balance. The outside diameter of the sphere is then measured, the thickness of the wall estimated, as well as the volume of the neck, and the volume of the air computed. Sometimes smaller, metallic spheres were used in this experiment. An example can be seen mounted on the vacuum pump.

6
Pressure Pressure is defined as force per unit area. It is usually more convenient to use pressure rather than force to describe the influences upon fluid behavior. The standard unit for pressure is the Pascal, which is a Newton per square meter. For an object sitting on a surface, the force pressing on the surface is the weight of the object, but in different orientations it might have a different area in contact with the surface and therefore exert a different pressure.

7
**Pressure calculations**

There are many physical situations where pressure is the most important variable. If you are peeling an apple, then pressure is the key variable: if the knife is sharp, then the area of contact is small and you can peel with less force exerted on the blade. If you must get an injection, then pressure is the most important variable in getting the needle through your skin: it is better to have a sharp needle than a dull one since the smaller area of contact implies that less force is required to push the needle through the skin. When you deal with the pressure of a liquid at rest, the medium is treated as a continuous distribution of matter. But when you deal with a gas pressure, it must be approached as an average pressure from molecular collisions with the walls. Pressure in a fluid can be seen to be a measure of energy per unit volume by means of the definition of work. This energy is related to other forms of fluid energy by the Bernoulli equation.

8
Pressure in liquids Liquids exert pressure due to distribution of their own weight. To see how liquids exert pressure, try the following experiment. Take three tins of different sizes or diameters. On tin number I, make three holes at the same height. On tin numbers II and III, make three holes at different heights. Place three long tapes to close the three holes on each on the tins. Now fill the tin with water. Remove the tapes quickly and observe the streams coming out of each of the holes. You will observe the following : Water stream will start pouring out through the holes. This means that water is exerting pressure in all direction. In tin I, the water stream comes out evenly irrespective of the direction of the hole. This means that the pressure is equal at the same height or depth. In Tin II and III, the water stream coming out of the lowest hole reaches the farthest. This shows that the pressure exerted by liquid increases with depth. Also the pressure is acting perpendicular to the liquid surface. Since there is no difference between the streams coming out of tins II and III, the pressure exerted by liquid is independent of the size of the container, but depends only on the height or the depth of the liquid. (This is markedly different from what happens when a solid is applying pressure or weight, as seen in the earlier section).

9
**Formula for Pressure in liquids**

10
**Pressure in the atmosphere**

Atmospheric pressure is the force per unit area exerted against a surface by the weight of air above that surface in the Earth's atmosphere. In most circumstances atmospheric pressure is closely approximated by the hydrostatic pressure caused by the weight of air above the measurement point. Low pressure areas have less atmospheric mass above their location, whereas high pressure areas have more atmospheric mass above their location. Similarly, as elevation increases there is less overlying atmospheric mass, so that pressure decreases with increasing elevation. A column of air one square inch in cross-section, measured from sea level to the top of the atmosphere, would weigh just over a stone (and a column one square centimetre in cross-section would weigh just over a kilogram). Standard Atmospheric Pressure Force per unit area exerted by the air above the surface of the Earth. Standard sea-level pressure, by definition, equals 1 atmosphere (atm), or in. (760 mm) of mercury, lbs per square in., or kilopascals, but pressure varies with elevation and temperature. It is usually measured with a mercury barometer (hence the term barometric pressure), which indicates the height of a column of mercury that exactly balances the weight of the column of atmosphere above it. It may also be measured using an aneroid barometer, in which the action of atmospheric pressure in bending a metallic surface is made to move a pointer.

11
Barometers A barometer is a scientific instrument used to measure atmospheric pressure. It can measure the pressure exerted by the atmosphere by using water, air, or mercury. Pressure tendency can forecast short term changes in the weather. Numerous measurements of air pressure are used within surface weather analysis to help find surface troughs, high pressure systems, and frontal boundaries. Water-based barometers It consists of a glass container with a sealed body, half filled with water. A narrow spout connects to the body below the water level and rises above the water level, where it is open to the atmosphere. When the air pressure is lower than it was at the time the body was sealed, the water level in the spout will rise above the water level in the body; when the air pressure is higher, the water level in the spout will drop below the water level in the body. A variation of this type of barometer can be easily made at home Mercury barometers A mercury barometer has a glass tube of at least 33 inches in height, closed at one end, with an open mercury-filled reservoir at the base. The weight of the mercury creates a vacuum in the top of the tube. Mercury in the tube adjusts until the weight of the mercury column balances the atmospheric force exerted on the reservoir. High atmospheric pressure places more force on the reservoir, forcing mercury higher in the column. Low pressure allows the mercury to drop to a lower level in the column by lowering the force placed on the reservoir. Since higher temperature at the instrument will reduce the density of the mercury, the scale for reading the height of the mercury is adjusted to compensate for this effect. The mercury barometer's design gives rise to the expression of atmospheric pressure in inches or millimeters: the pressure is quoted as the level of the mercury's height in the vertical column. 1 atmosphere is equivalent to about 29.9 inches, or 760 millimeters, of mercury. Barometers of this type normally measure atmospheric pressures between 28 and 31 inches of mercury.

12
manometers A manometer measures the difference in air or liquid pressure by comparing it to an outside source, usually a sample of Earth's atmosphere. Common manometers are U-shaped and have interconnected tubes. Manometers are used in atmospheric surveys, weather studies, gas analyses and research of the atmospheres of other planets. They are usually made of glass or plastic, and while most are scored for measurement, some can measure changes digitally. The single-tube manometer measures only the pressure of a liquid, since there is no alternate place to compare gases. A U-shaped manometer essentially pits two different gas pressures against one another, and measures the strength of the captured gas. The free-flowing gas is usually air at the current atmospheric level. How it works A liquid is placed in the tube, usually a responsive liquid like mercury that is stable under pressure. One end of the U-tube is then filled with the gas to be measured, usually pumped in so the tube can be sealed behind it. The other end is left open for a natural pressure level. The liquid is then balanced in the lower section of the U, depending on the strength of the gas. The atmospheric pressure pushes down on the liquid, forcing it down and into the closed end of the tube. The gas trapped in the sealed end also pushes down, forcing the liquid back to the other side. Then a measurement is taken to see how far the liquid in the sealed end has been pushed either below the point of the liquid in the open end or above it. If the liquid is level, straight across in both tubes, then the gas is equal to outside air pressure. If the liquid rises above this level in the sealed end, then the air's pressure is heavier than the gas. If the gas is heavier than the air, it will push the liquid in the sealed end below the equal point.

13
**Kinetic theory of matter**

Assumptions of theory The Kinetic Theory of Matter is a prediction of how matter should behave, based on certain assumptions and approximations. The assumptions are made from observations and experiments, such as the fact that materials consist of small molecules or atoms. Approximations are made to keep the theory from being too complex. One assumption is that the size of the particles is so small that it can be considered a point. Matter consists of small particles The first assumption in this theory is that matter consists of a large number a very small particles—either individual atoms or molecules. Large separation between particles The next assumption concerns the separation of the particles. In a gas, the separation between particles is very large compared to their size, such that there are no attractive or repulsive forces between the molecules. In a liquid, the particles are still far apart, but now they are close enough that attractive forces confine the material to the shape of its container. In a solid, the particles are so close that the forces of attraction confine the material to a specific shape.

14
**Particles in constant motion**

Another assumption is that each particle is in constant motion. In gases, the movement of the particles is assumed to be random and free. In liquids, the movement is somewhat constrained by the volume of the liquid. In solids, the motion of the particles is severely constrained to a small area, in order for the solid to maintain its shape. The velocity of each particle determines its kinetic energy. Collisions transfer energy The numerous particles often collide with each other. Also, if a gas or liquid is confined in a container, the particles collide with the particles that make up the walls of a container. No energy change Thus, an assumption is that the particles transfer energy in a collision with no net energy change. That means the collisions between the particles are perfectly elastic and no energy is gained or lost during the collision. This follows the Law of the Conservation of Energy. In reality, the collisions are not perfect, and some energy is lost. But for the sake of simplicity in drawing conclusions, this theory makes the collisions elastic.

15
**The gas laws BOYLE’S LAW**

Boyle's law is one of many gas laws and a special case of the ideal gas law. Boyle's law describes the inversely proportional relationship between the absolute pressure and volume of a gas, if the temperature is kept constant within a closed system. The law was named after chemist and physicist Robert Boyle, who published the original law in The law itself can be stated as follows: For a fixed amount of an ideal gas kept at a fixed temperature, P [pressure] and V [volume] are inversely proportional (while one increases, the other decreases). The mathematical equation for Boyle's law is: where: p denotes the pressure of the system. V denotes the volume of the gas. k is a constant value representative of the pressure and volume of the system. So long as temperature remains constant the same amount of energy given to the system persists throughout its operation and therefore, theoretically, the value of k will remain constant. However, due to the derivation of pressure as perpendicular applied force and the probabilistic likelihood of collisions with other particles through collision theory, the application of force to a surface may not be infinitely constant for such values of k, but will have a limit when differentiating such values over a given time. Forcing the volume V of the fixed quantity of gas to increase, keeping the gas at the initially measured temperature, the pressure p must decrease proportionally. Conversely, reducing the volume of the gas increases the pressure. Boyle's law is used to predict the result of introducing a change, in volume and pressure only, to the initial state of a fixed quantity of gas. The before and after volumes and pressures of the fixed amount of gas, where the before and after temperatures are the same (heating or cooling will be required to meet this condition), are related by the equation:

16
CHARLES’S LAW A modern statement of Charles's law is: At constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature on the absolute temperature scale (i.e. the gas expands as the temperature increases). which can be written as: where V is the volume of the gas; and T is the absolute temperature. The law can also be usefully expressed as follows: The equation shows that, as absolute temperature increases, the volume of the gas also increases in proportion. PRESSURE LAW The pressure of a fixed mass of gas is directly proportional to absolute temperature, provided the volume of gas is constant. P Or P/T = constant P1/ T1 = P2/ T2

Similar presentations

OK

The Behavior of Gases Chapter 14. Chapter 14: Terms to Know Compressibility Boyle’s law Charles’s law Gay-Lussac’s law Combined gas law Ideal gas constant.

The Behavior of Gases Chapter 14. Chapter 14: Terms to Know Compressibility Boyle’s law Charles’s law Gay-Lussac’s law Combined gas law Ideal gas constant.

© 2018 SlidePlayer.com Inc.

All rights reserved.

Ads by Google

Ppt on service oriented architecture example Free download ppt on statistics for class 11 Ppt on obesity management dog Ppt on water conservation techniques Ppt on food processing technology Ppt on polynomials download music Ppt on different types of forests in world Ppt on kingdom monera organisms Ppt on total parenteral nutrition complications Ppt on solar energy projects in rural america