1 1 1 1 1 A Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 B C Total Pressure (kPa) Air Pressure (kPa) 104.40 99.67 108.51 101.84 111.47 103.36 113.79 104.00 115.89 104.61 D Temperature (oC) 21.2 27.6 32.1 34.0 35.8 E Temp(k) 294.35 300.75 305.25 307.15 308.95 Calculate the natural logarithm of the vapor pressures, In(P/P), where P is 100 kPa. Prepare a graph (either by hand or in Excel) with In (P/P) plotted on the y-axis and 1/T (K-¹) plotted on the x- axis. Follow all the rules for properly preparing a scientific graph. Remember to turn in your graph with your report. Determine the line of best fit for your data. Calculate the slope of this line. From the slope calculate the enthalpy of vaporization. F 1/T(k^-1) 0.00339 0.00332 0.00327 0.00325 0.00323 G vapour pressure(kpa) 4..73 6.67 8.11 9.79 11.28 H In(p/p0) Enthalpy of vaorisation

1 1 1 1 1 A Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 B C Total Pressure (kPa) Air Pressure (kPa) 104.40 99.67 108.51 101.84 111.47 103.36 113.79 104.00 115.89 104.61 D Temperature (oC) 21.2 27.6 32.1 34.0 35.8 E Temp(k) 294.35 300.75 305.25 307.15 308.95 Calculate the natural logarithm of the vapor pressures, In(P/P), where P is 100 kPa. Prepare a graph (either by hand or in Excel) with In (P/P) plotted on the y-axis and 1/T (K-¹) plotted on the x- axis. Follow all the rules for properly preparing a scientific graph. Remember to turn in your graph with your report. Determine the line of best fit for your data. Calculate the slope of this line. From the slope calculate the enthalpy of vaporization. F 1/T(k^-1) 0.00339 0.00332 0.00327 0.00325 0.00323 G vapour pressure(kpa) 4..73 6.67 8.11 9.79 11.28 H In(p/p0) Enthalpy of vaorisation

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section8.7: Kinetic-molecular Theory And The Velocities Of Gas Molecules

Problem 8.12PSP

See similar textbooks

Similar questions

How would the use of a volatile liquid affect the measurement of a gas using open-ended manometers vs. closed-end manometers?
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
In an experiment in a general chemistry laboratory, a student collected a sample of a gas over water. The volume of the gas was 265 mL at a pressure of 753 torr and a temperature of 27 C. The mass of the gas was 0.472 g. What was the molar mass of the gas?
A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2, is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O2 in the balloon? (d) What is the mole fraction of each gas?
A typical barometric pressure in Redding. California, is about 750 mm Hg. Calculate this pressure in atm and kPa.
A typical barometric pressure in Kansas City is 740 torr. What is this pressure in atmospheres, in millimeters of mercury, and in kilopascals?
5-107 If 60.0 g of NH3 occupies 35.1 L under a pressure of 77.2 in. Hg, what is the temperature of the gas, in °C?
A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25C and the barometric pressure is 730 torr. The balloon then rises to an altitude of 6000 ft, where the pressure is 605 torr and the temperature is 15C. What is the change in volume of the balloon as it ascends from sea level to 6000 ft?