The ambient temperature is 85.0°F and the humidity of the surrounding air is reported to be 62.0%. Using the Clausius-Clapeyron equation and the boiling point of water as 100.0°C at 760.0 torr, calculate the vapor pressure (in torr) of water in the air. Use 40.7 kJ/mol as the ∆Hvap of water.

Suppose you have a perfectly insulated container holding 2.00 kg of liquid water at a temperature of 20.0°C. You also have a large supply of ice cubes which are stored at a temperature of-20.0°C. (a) What is the maximum mass of ice you can add to the water so that all of the ice melts? Assume no heat is lost to the environment. (b) Suppose you add twice the mass of ice that you found in part a. How much solid ice will remain once thermal equilibrium is reached?

The enthalpy of vaporization for methanol is 35.2 kJ/mol. Methanol has a vapor pressure of 101.3 kPa at 64.7 °C. Using the Clausius-Clapeyron equation, what is the vapor pressure for methanol at 44.9 °C? Give your answer in kPa, to the first decimal point.

Two 20.0 g ice cubes at -17.00C are placed into 470.1 g of water at 25.0 0C. The heat of fusion of ice is 6.008 kJ/mol, the molar heat capacity of water is 75.3 J mol-1 K-1 and the molar heat capacity of ice is 37.7 J mol-1 K-1. Assuming no energy is transferred to or from the surroundings, please calculate the final temperature of the water after all the ice melts. _______ 0C

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.05  kg of water decreased from 117  °C to 56.5  °C.  Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C

The normal boiling point of mercury (Hg) is 356.7 °C. What is the vapor pressure of mercury at 317.0 °C in atm? (AHvap = 58.51 kJ/mol)

What is the vapor pressure of SiCl4 in mmHg at 27.5∘C? The vapor pressure of SiCl4 is 100 mmHg at 5.4∘C, and ΔHvap = 30.2 kJ/mol.

The enthalpy of vaporization for methanol is 35.2 kJ/mol. Methanol has a vapor pressure of 101.3 kPa at 64.7 °C. Using the Clausius-Clapeyron equation, what is the vapor pressure for methanol at 37.7 °C? Give your answer in kPa, to the first decimal point.

Suppose the boiling point of pure water at high altitude is 85.00 °C. Use the Clausius-Clapeyron equation to determine the atmospheric pressure at this high altitude. The normal boiling point of water is 100.0 °C at 1 atm and its heat of vaporization is 40.7 kJ/mol.

The normal boiling point of mercury (Hg) is 356.7 °C. What is the vapor pressure of mercury at 340.0 °C in atm? (∆Hvap = 58.51 kJ/mol)