In this lab, you will start off by calculating the number of moles of air molecules inside a flask containing 20 mL of water by cooling the flask down to near 0°C and assuming the vapour pressure of water is negligible at that temperature. If the volume of the air inside the flask is 145.8 mL, the gas pressure sensors reads 101.7 kPa and the temperature sensor reads 3.7 °C, how many moles of air are present in the flask? Express your answer in mol. Assume R = 8.314 J mol-1 K-1.

Calculate the partial and total pressures of the vapor over a mixture of 3 moles of CHCl3 and 1 mol of heptane at 60OC. CHCl3 vapor pressure is 800mmHg and Heptane vapor pressure is 200mmHg.

A volume of 7.32 L of air is bubbled through liquid toluene at 360. K, thus reducing the mass of toluene in the beaker by 11.2 g. Assuming that the air emerging from the beaker is saturated with toluene, determine the vapor pressure of toluene at this temperature.

The normal boiling point of cyclohexane is 80.74 °C.At 20.00 °C, the vapour pressure of cyclohexane is 0.1026 atm.What is the vapour pressure of cyclohexane when the temperature is 33.00 °C? ----------------------------------------------------------------------------------- The vapour pressure at the normal boiling point is known, by definition, to be 1 atm.You therefore can write three different equations of the sort:lnPvap = [(−∆H)/(RT)] + Ci.e. for each of the three pairs of P and T.You can take the difference between the equations for the cases (Pb, Tb) and (P1, T1).This could be used to solve for [(−∆H)/(R)].Analogously you can take the difference between the equations for the cases (Pb, Tb) and(P2, T2).Since both differances must give rise to the same value for [(−∆H)/(R)], you can equate them to write an equation which allows you to calculate P2 in terms of Pb, Tb, P1, T1 and T2