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3. Calculate the number of moles of air molecules trapped in your flask using the Ideal Gas Law (PV = nRT). Remember to watch your units, and that R = 8.314 J mol-1 K-1 = 0.0821 atm L mol-1 K-1 = 0.0831 bar L mol-1 K-1. Show your work for the above calculation. ANSWERED: Number of moles of air molecules? P= 100.7 kPa T= 275.85 V=20 mL Changing units: V= 20 x 10^-3 L P= 100.7/100= 0.9938 atm PV= nRT PV/RT=n 0.9938x20x10^-3/0.0821x275.85 = 8.776x10^-4 moles= n 4. Complete the following table to calculate the vapour pressure of your liquid at each of the three experimental temperatures. Remember to recalculate the pressure of the air molecules using the Ideal Gas Law. Use Dalton's Law to calculate the vapour pressure of your liquid. Temperature (k) | Pressure Reading P experimental, kPa | Pressure from Air Molecules (P air, kPa | Vapour Pressure of your Liquid (P vapour, kPa 5. Transform your experimental data from the previous table as shown below (for all three experimental temperatures). The data must be transformed in order to fit it to the Clausius-Clapeyron equation.

          3. Calculate the number of moles of air molecules trapped in your flask using the Ideal Gas Law (PV = nRT). Remember to watch your units, and that R = 8.314 J mol-1 K-1 = 0.0821 atm L mol-1 K-1 = 0.0831 bar L mol-1 K-1.

Show your work for the above calculation.

ANSWERED: Number of moles of air molecules?
P= 100.7 kPa
T= 275.85
V=20 mL
Changing units:
V= 20 x 10^-3 L
P= 100.7/100= 0.9938 atm
PV= nRT
PV/RT=n
0.9938x20x10^-3/0.0821x275.85
= 8.776x10^-4 moles= n

4. Complete the following table to calculate the vapour pressure of your liquid at each of the three experimental temperatures. Remember to recalculate the pressure of the air molecules using the Ideal Gas Law. Use Dalton's Law to calculate the vapour pressure of your liquid.

Temperature (k) | Pressure Reading P experimental, kPa | Pressure from Air Molecules (P air, kPa | Vapour Pressure of your Liquid (P vapour, kPa

5. Transform your experimental data from the previous table as shown below (for all three experimental temperatures). The data must be transformed in order to fit it to the Clausius-Clapeyron equation.

3. Calculate the number of moles of air molecules trapped in your flask using the Ideal Gas Law (PV = nRT). Remember to watch your units, and that R = 8.314 J mol-1 K-1 = 0.0821 atm L mol-1 K-1 = 0.0831 bar L mol-1 K-1.

Show your work for the above calculation.

ANSWERED: Number of moles of air molecules?
P= 100.7 kPa
T= 275.85
V=20 mL
Changing units:
V= 20 x 10^-3 L
P= 100.7/100= 0.9938 atm
PV= nRT
PV/RT=n
0.9938x20x10^-3/0.0821x275.85
= 8.776x10^-4 moles= n

4. Complete the following table to calculate the vapour pressure of your liquid at each of the three experimental temperatures. Remember to recalculate the pressure of the air molecules using the Ideal Gas Law. Use Dalton's Law to calculate the vapour pressure of your liquid.

Temperature (k) | Pressure Reading P experimental, kPa | Pressure from Air Molecules (P air, kPa | Vapour Pressure of your Liquid (P vapour, kPa

5. Transform your experimental data from the previous table as shown below (for all three experimental temperatures). The data must be transformed in order to fit it to the Clausius-Clapeyron equation.

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