'Vapor Pressure and Heat Evaporation Lab Report\r'

' dehydration storm and Heat of Vaporization Introduction: ? vapor is the process of a eloquent becoming vaporized. When a quiet is placed into a confined lacuna some of the luculents pull up stakes evapo come in. Evaporation of the liquid depends on the strength of the intermolecular forces that argon between liquid molecules. During the evaporation process of the liquid, new gasconade molecules exerts press in the sealed container, while some of the gas condenses back down to the liquid state. ?If the temperature inside the container is kept eternal, indeed the chemical equilibrium at some point ordain be reached.When the equilibrium is reached, the rate of condensation is check to the rate of evaporation and the rate of vapor tweet go out remain constant as recollective as the temperature in the sealed container does non change. ?The alliance between the vapor force per unit ara of a liquid and temperature is described in the Clausius-Clayperon equation: lnP= ? Hvap / R (1/T)+C. where 1nP is the inbred logarithm of the vapor squelch, ? Hvap is the change in hot up vaporization, R is the universal gas constant, which is (8. 31 J/mol•K), T is the absolute, or Kelvin, temperature, and C is the constant that is not related to heat capacity.Therefore, Clausius-Clayperon equation does not only describes how vapor pressure is affected by the temperature, but relates to the factors of heat vaporization of a liquid. ?The single-valued function of this experiment is to determine the relationship between the pressure and temperature of the volatile liquids. The pressure will be mensural in a sealed vessel that contains dissimilar types of liquids such as methanol, ethanol and propanol. It will be measured several times at various temperatures. At the conclusion of this experiment, the heat of vaporization will be subject to be calculated.Materials: ?To be able to complete this lab procedure, the materials that be needed is a Vernier computer interface, a Vernier particle accelerator Pressure Sensor, temperature probe, rubber ballyhoo assembly, plastic provide with two drawors, hot ordered series, ice, one twenty milliliter syringe, one 400 milliliter beaker, two one hundred twenty-five milliliter Erlenmeyer flaskfuls, one 1 liter beaker, ethanol, methanol, and 1-propanol. Methods: ?The commencement exercise gradation in performing this experiment is to recover and wear goggles. The alcohols theatrical roled in this experiment are flammable and poisonous.The second bar is to obtain the materials that are needed and set them up as accordingly. The threesome step is to use a hot plate to heat 200 milliliters of water in a 400 milliliter beaker. The fourth step is to bring in a room temperature water bathe in a 1 liter beaker. The fifth part step is to connect the Gas Pressure Sensor to furrow one of the Vernier computer interface, consequently connect the Temperature Probe to channel two of the interface and then connect it to a computer. The sixth step is to use the clear tubing to connect the white stopper to the Gas Pressure Sensor.The white stopper moldiness be twisted snugly into the neck of the Erlenmeyer flask, to invalidate losing any of the gas that will be produced when the liquid starts evaporating. The most important thing to do is to recommend to faithful the valve on the white stopper. ?The seventh step is to draw in 3 milliliters of methanol into the 20 milliliter syringe that is part of the Gas Pressure Sensor accessories. Place the syringe onto the valve of the white stopper. The eighth step is to start the Logger Pro weapons platform and open the file â€Å"34 Vapor” from the innovative Chemistry with Vernier folder. The ninth step is to get through â€Å"collect” to begin collecting data.The first measurement will be the pressure of the air in the flask and the room temperature. Place the Temperature Probe secretive the flask. When the pressure and temperature readings are stabilized, click â€Å"keep” to express the readings. The tenth step is to add methanol to the flask by opening the valve below the syringe, push good deal on the syringe to inject the 1-propanol and quickly close the valve. Afterwards, remove the syringe from the stopper and monitor the pressure and temperature readings. ?The eleventh step is to place the stoppered flask into the 1 liter beaker of room temperature water.Place the Temperature Probe in the water bath and monitor the pressure and temperature readings. The 12th step is to add a small list of hot water to warm the water bath by only a few degrees. submit the water with the temperature probe and monitor the pressure and temperature readings. For the 13th step, repeat step twelve until five streamlets are completed. Add hot water for each streamlet so the temperature of the water bath increases. After the fifth trail is go ined, open the valve to release the pres sure in the flask and dispose of the alcohol as directed.The 15th step is to end the data collection and disk the pressure and temperature readings in the data table. When recording the data, record the pressure valve of the first data point as Pair for trials one and two and record the temperature for trial one. Record the pressure value of the second data point as Ptotal for trial two as well as the temperature. The remaining values are recorded as Ptotal for trial two as well as the appropriate temperature. The last and nett step is to clean the work area. Data add-in: Methanol Trial 1 Trial 2 Trial 3 direct 4 domicile 5 Ptotal (mmHg) 103. 1 04. 5 105. 8 101. 9 Pair (mmHg) 101. 3 102. 4 103. 3 104. 4 105. 2 Pvap (mmHg) 0. 7 1. 2 1. 4 2. 7 Temperature (Celsius) 22. 6 25. 8 28. 3 31. 2 34. 0 Ethanol Trial 1 Trial 2 Trial 3 cartroad 4 Trail 5 Ptotal (mmHg) 106. 3 94. 7 98. 9 112. 9 Pair (mmHg) 100. 8 100. 8 92. 78 96. 0 103. 4 Pvap (mmHg) 5. 4 1. 92 2. 9 9. 5 Temperature (Cels ius) 23. 9 24. 0 0. 3 9. 9 31. 7 Propanol Trial 1 Trial 2 Trial 3 Trail 4 Trail 5 Ptotal (mmHg) 101. 7 104. 9 106. 1 108. 3 Pair (mmHg) 100. 4 101. 1 102. 2 103. 1 104. 0 Pvap (mmHg) 0. 6 2. 7 3. 0 4. 3 Temperature (Celsius) 23. 8 23. 7 0. 2 6. 5 29. 1 Discussion At the end of this experiment, the results we obtained varied because of the incompatible temperatures and pressures that we observed. During the evaporation process of the liquid, gas molecules exerts pressure in the sealed container, while some of the gas condenses back to the liquid state. If the temperature inside the container is kept constant, then the equilibrium was reached. When the equilibrium is reached, the rate of condensation is equal to the rate of evaporation and the rate of vapor pressure will remain constant as long as the temperature in the sealed container does not change.\r\n'