Predict the sign of q for the process of water vapor condensation. 0 >b q >0 q =D0 Predict the sign of w for the process of water vapor condensation. w<0 w >0

Dry nitrogen gas (100.0 L) was bubbled through liquid ethanol, C2H5OH, at a given temperature and the evaporated ethanol condensed; its mass was then measured. Using the data below, calculate the heat of vaporization (kJ/mol) of ethanol?

Calculate the enthalpy of vaporization of SO2 at –25°C if the same at its boiling point (i.e. –10°C) be 5950 cal mol–1. Given for SO2, molar heat capacities in liquid and vapor phase are 206 cal K–1 mol–1 and 9.3 cal K–1 mol–1 respectively.

The pressures deep within the Earth are much greater than those on the surface, and to make use of thermochemical data in geochemical assessments you need to take the differences into account. (a) Given that the enthalpy of combustion of graphite is -393.5 kJ mol-1 and that of diamond is -395.41 kJ mol-1, calculate the standard enthalpy of the C(s, graphite) → C(s, diamond) transition. (b) The densities of graphite and diamond are 2.250 g cm-3 and 3.510 g cm-3 , respectively. Calculate the internal energy of the transition when the sample is under a pressure of 150 kbar.

To vaporize 100.0 g carbon tetrachloride at its normal boiling point, 349.9 K, and P =1 atm, 19.5 kJ of heat is required. Calculate DHvap for CCl4 and compare it with DU for the same process.

The enthalpy of vaporization of chlorine at the standard (1 atm) boiling point (284 K) is 20.41 kJ/mol. What is the change in internal energy when one mole of chlorine vaporizes under those conditions?

A thermally insulated container (closed system) is dropped from a certain height andfilled with water so that it collides inelastically against the ground. what should be the valueof the height in m so that the temperature of the water increases by 0.5 °C? Suppose thatall the energy lost in the fall is invested in increasing the temperature of the water.I considered a gravitational acceleration of 9.81 m/s2.

For an ideal gas P= nRT/V, and for a gas whose molecules have volume  P=nRT/(V-nb)  How would you modify this latter equation for a real gas to correct for the fact that there are attractive forces between molecules.

The following is a table of water vapor pressure in millibar (mbar) vs Temp in oC.  In your own words, explain what equilibrium this represents, making sure to include an equation, and why it changes with temperature.     T (°C) P (mbar) 15 17.1 16 18.1 17 19.3 18 20.7 19 22.0 20 23.3 21 24.9 22 26.4 23 28.1 24 29.9 25 31.7 26 33.6 27 35.6 28 37.7 29 40.0 30 42.4

What is the change in the boiling point of water at 1000 C per Pa change under atmospheric pressure conditions? The molar enthalpy of vaporization is 40.69 kJ mol-1, the molar volume of liquid water is 0.019 x 10-3 m3 mol-1, and the molar volume of steam is 30.199 x 10-3m3 mol-1, all at 100.000 C and 1.01325 bar. (Hint: change in temperature per change in pressure, dT/dP).