Vapor pressure Essays

. Introduction Vapor pressure is the tendency of the liquid to evaporate and the amount of gas at equilibrium, while vapor is when molecules move from a liquid phase to a gaseous state. Vapor is basically what liquid produces after it starts evaporating. Liquids evaporate because some portions of their molecules have sufficient energy to flee from the liquid phase and become vapor. Some liquids even evaporate faster than other liquids. This is because some of these liquids can be more volatile

tested vapor pressure, viscosity, and surface tension. The vapor pressure was tested by putting a drop of the liquid on the laminated paper and waiting 30 second to see which one had reverberated. The viscosity was tested by putting a drops of different liquids on the laminated paper and holding the paper vertically to see which one fell the fastest. The surface tension was tested by how far the liquid spread when a drop of it was put on the laminated paper. The propanol had a high vapor pressure

Vapor Pressure of Water vs. Temperature Use your observations from the pressure vs. temperature lab to answer the following questions: 1. What happened to the height of the water according to your lab investigation? I should see the terms vapor pressure and temperature properly used. 2. What happened to the vapor pressure of water as the temperature increased? 3. In your lab, you noticed that the height of the water changed as you increased the water temperature. Barometers work in a similar

PREPARATION AND USES OF SODIUM HYDROXIDE, BLEACHING POWDER, BAKING POWDER, WASHING SODA Objective: To understand the use of common salt (NaCl) for preparation of chemicals such as Sodium hydroxide, Bleaching powder, Baking powder, Washing soda. The common salt (Chemical formula-NaCl, Chemical name- Sodium chloride) that we eat in our daily diet is the raw material for preparation of chemical compounds such as Sodium hydroxide, Bleaching powder, Baking powder, Washing soda. NaCl is a neutral salt

AIM Design an experiment to study a thermodynamic property of a chemical substance, a chemical reaction, a physical change or chemical phenomenon. BACKGROUND INFORMATION Standard enthalpy change of solution, ∆Hsolnø, is the enthalpy change when one mole of a substance dissolves in water to form a solution of infinite dilution under standard conditions.1 The standard enthalpy change can either be exothermic or endothermic. An exothermic reaction is a reaction where energy is released as a form of

The Mpemba effect is that, under certain circumstances and experimental parameters, it is observed that hot water freezes faster than cold water which sounds implausible since hot water, with a higher temperature than cold water, has a higher amount of internal energy which has to be lost before it starts to change its state and turn into ice. The effect got its name from Erasto Mpemba who discovered the effect that hot water freezes faster than cold water after he discovered that hot ice-cream freezes

from vaporization is known as vapor and it is assumed to behave as an ideal gas. One of the properties that characterize a volatile liquid is determination of its molar mass. Dumas method also known as the vapor density method uses the vapor density of the unknown volatile liquid in determining its molar mass. The major assumptions of these methods are the substance behaves ideally. The molar mass of a volatile liquid can be obtained by measuring the temperature, pressure, mass, and volume in a gaseous

Determining the Molar Volume of a Gas Lab Report The purpose of the experiment is to determine the molar volume of hydrogen gas at standard pressure and temperature. Excess hydrochloric acid was placed in a eudiometer and decanted with deionized water. A piece of magnesium ribbon was trapped in a copper wire cage in the eudiometer in order to keep it in place as the more dense hydrochloric acid diffused downward in the inverted eudiometer. The eudiometer was placed in a water bath and the magnesium

produced are a salt in aqueous solution and a gas. While the salt remains in the water as part of a solution, the gas produced will float to the top. Though water vapor pressure will affect the pressure of the gas in the eudiometer, it is possible to apply Dalton’s law of partial pursues to find the dry pressure of the gas. When the dry pressure is determined, the volume of the gas at STP can then be determined and what the experimental volume of one mole of the gas would be at STP. 1. Put on the necessary

When you collect the gas through the eudiometer, the water inside the eudiometer gets displaced, evaporating until the pressure of the water outside is equal to the pressure inside. To correctly find the pressure of the gas, the pressure of the water vapor must be subtracted, as the two are mixed together. What is the limiting reactant for the reaction? What is the experimental evidence that you are basing it on? Based on the experimental

that an upward force acts on an object when submerged in a gas or liquid.[1] When the object is at rest, this force, called the buoyant force, is equal and opposite to the force acting downwards on the object.[1] The buoyant force is caused by the pressure of the gas or liquid the object is in and increases the further down the object is in the fluid, as described by Boyle’s Law. This can be seen in the image below where a five kilogram weight has a buoyant force of 2 kilograms acting upon it. This

needed to be measured, like the pressure of the room, the molar mass of the gas, the volume of the gas, and the temperature of the water the gas was in. First, the volatile liquid was heated up until it evaporated. After collecting the required data, calculations were done to determine the molar mass of the compound. Key terms used in this lab are the ideal gas law, PV = nRT, which was used in finding the molar mass. Another term is vapor pressure, which is the pressure exerted by a liquid in gaseous

Converting the recorded room pressure from inches Hg to millimeters Hg in order to find the total pressure to plug into Pressure Conversion and Adjustment equation, which finds the pressure of H2. (** use the water vapor pressure chart in order to find the pressure of water)

to determine the molar mass of a volatile gas by using the ideal gas law. Procedure: First a 600 mL beaker was filled half way with water and assembled into a boiling water bath. Then 2 stoppers were obtained, one had a hole at the top so that vapor could easily flow out. The stopper with the hole was then placed on a flask. 2.5 mL of unknown liquid B was then put into the flask with the stopper containing a hole in the top. This beaker was then placed in the boiling water bath with a thermometer

One common misrepresentation of wintertime is the structure of a snowflake. Snowflakes are most likely depicted and drawn as having eight sides, but in actuality snowflakes have six sides which is something that not many people are aware of. Proving this fact can be as simple as collecting a sample of falling snow and viewing it under a microscope. The basis of a snowflake, and its hexagonal shape, is etched down to what holds it together: ice crystals. The atmosphere contains a plethora of ice crystals

Up in the clouds on a cold Winters day, water vapor condenses into a water droplet and freezes into a tiny specs of dust. The water molecules morph together as a hexagonal pattern. As the water vapor condenses on the surface and the ice crystal grows larger and small branches bud off the hexagonal ice design. The ice crystal grows heavy enough it falls to the ground and is called and is then called a snowflake. This process happens over and over millions of times during a snowstorm. They are formed

athletes taking part in the risk culture are lifestyle choices. Athletes taking part in sport specific risk behaviours for victory is becoming a social health problem. The risks taken to search for the normalized image are because of social and self pressures as well as the use of performance enhancing drugs. We see in everyday life that athletes are pushing themselves to strive for victory, and a reason for this is because they feel pressured from society. People are continuing to search for the ideal

Volume and Temperature of a Gas By: Jasmine Camacho In this experiment I used both the Boyle’s and the Charles gas laws. Boyle's law states “the volume of a given quantity of a gas varies inversely as the pressure, the temperature remaining constant”. The formula used to help complete this process is PV=constant. Charles law help explain the relationship between temperature and gas volume. And the formula for this is V/T=constant. For this experiment I used the ideal gas law; pV=nRT.

states that the number of moles are proportional to the volume of a gas at a constant temperature and pressure. V = kn where k is the constant of proportionality. Avogadro introduces the idea of particles and how they combine and react in a chemical reaction. A soft drink is an example of Avogadro’s law. When the soft drink is shaken molecules will be released into the air. Therefore the pressure in the bottle is proportional to the number of moles of molecules in the bottle. Boyle’s Law published

“P1V1 = P2V2” shows that as the volume increases, the pressure of the gas decreases in proportion, as long as the temperature stays the same. The relationship between pressure and volume was first noticed by mathematician and astronomer Richard Towneley and experimenter Henry Power. Robert Boyle, a chemist and physicist, confirmed the discovery and published the results in 1662. According to science historians, Boyle’s assistant, Robert Hooke, built the experimental rig. The law is based on air