write subtracted be was THE DATA Kelvin must PROCESSING Celsius to air temperatu
ID: 483389 • Letter: W
Question
write subtracted be was THE DATA Kelvin must PROCESSING Celsius to air temperature, dair the temperatures the pressure must Convert for to a higher law However, due obtain the v pressure values. gas use the To of measured would To this, due to a l in 2, or do the the bath Trial 3, convert of water domGase Kelvin of Trial 1 the be and the in Trial 2, 3, or Solve for Pr and are the atmospheric the water bath For Trial 1 trials, where water bath. T2 is temperature for 3, and 4. two for these record this not to make a correction; air methanol and Trial ethanol, it is in the blank measured the atmospheric value from the (and pressure 3. obtain the vapor pressure by subtracting the corrected air pressure methanol in Trials Subtract the uncorrected air pressure 1 of Trial l of ethanol from the measured pressure. collected for graph vapor temperature (oc)for the four data pairs you Note: Be methanol is the independent variable and vapor pressure is the dependent variable. As directed by your teacher, the graph manually, or use Logger Pro. sure to plot the vapor pressure, not the measured pressure. 5. would you describe the relationship between vapor pressure and temperature, as the represented in the graph you made in the previous step? Explain this relationship using concept kinetic energy of molecules. 6 Which liquid, methanol or ethanol, had the larger vapor value at room temperature? Explain your answer. Take into account various intermolecular forces in these two liquidsExplanation / Answer
(5)
The graph you obtain from your experimental data should show a non-linear increase in vapor pressure with respect to temperature.
This happens because as the temperature of the liquid increases, the average kinetic energy possessed by the molecules also increases. This increases the chance of more molecules having the required energy to escape out from the liquid into the gaseous phase.
Thus, vapor pressure increases with temperature.
(6)
Since methanol has a lower MW as compared to ethanol, so the Van Der Waal's intermolecular attractive forces are also less in methanol. So it's easier for the molecules of methanol to go from the liquid phase into the vapor phase because the energy requirement for this phase transition is comparitively less than ethanol.
Thus, methanol has higher vapor pressure than ethanol.
For making a plot as well as filling the table, you must provide experimental data related to it.
Revert back if you have any queries.
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