A compound has a vapor pressure of 92.1 torr(or mm Hg) at 35.2. \deg C. What is the normal boiling point of the compound? The enthalpy of vaporization of the compound is 31.77 kJ/mol., R = 8.3145 J/mol K. Make sure to convert temperature to Kelvin

In Boise, Idaho, the typical atmospheric pressure is 685 torr. What is the boiling point of water (AH, 370.4 vap K What pressure would have to be applied to steam at 373°C to condense the steam to liquid water? 194. X atm = 40.7 kJ/mol) in Boise? (Assume the normal boiling point of water is 100. °C.)

The enthalpy of vaporization for methanol is 35.2 kJ/mol. Methanol has a vapor pressure of 1 atm at 64.7 oC. Using the Clausius-Clapeyron equation, what is the vapor pressure for methanol at 46.3 oC? Give your answer in atmospheres, to the third decimal point.

carbon disulfide Cs2 has a heat of vaporization of 29,200 J/mol. at 268 K it has a vapor pressure of 1.0 X 10^2 mmHg. what is its vapor pressure at 301 K

1. Calculate the amount of heat (in kJ) released when converting 150.2 g of water to ice at -23 degrees Celsius.    2. A closed vessel of volume 10.0 L initially contains 1.303 g of water and no water vapor. Please calculate the mass of liquid water remaining once the system reaches equilibrium at 30 degrees Celsius. The vapor pressure of water at that temperature is equal to 0.0418 atm.   3. A person drinks four glasses of cold water (5 degrees C) every day. The volume of each glass is 195. mL. How much heat (in kJ) does the body have to supply to raise the temperature of the water to 37 degrees C (body temperature)?   4.From these data: N2H4(l) + O2(g) à 2N2(g) + 2H2O(l) H= -622.2 kJ/mol H2(g) + ½O2 à H2O(l) H= -285.8 kJ/mol H2(g) + O­2(g) à H2O2(l) H= -115 kJ/mol Find H for the reaction:                 N2H4(l) + 2H2O2(l) à 2N2(g) + 4H2O(l)   5. Consider the following chemical equation. CH4(g) + 2O2(g) à CO2(g) + 2H2O(l)                 Using the values in the table, calculate…

The vapor pressure of ethanol is 1.00 x 10“ mmHg at 34.90°C. What is its vapor pressure at 59.75°C? ( AHan for ethanol is 39.3 kJ/mol.) vap mmHg

Steam at 100oC was passed into a flask containing 276.87g of water at 21oC, where steam condensed. How many grams of steam must have condensed if the temperature of water in the flask was raised to76.1oC? The heat of vaporization of water (delta H) at 100oC is 40.7 kJ/mol and the specific heat is 4.18 J/g.oC.

The enthalpy of vaporization of Substance X is greater than that of Substance Y. Which of the following statements is true? O At any temperature where both substances are liquid, substance X will have the higher vapor pressure O At 1 atm pressure, substance Y will have the higher boiling point O At any temperature where both substances are liquid, substance Y will have the lower vapor pressure Substance Y would have IMF's with a greater magnitude than substance X O At 1 atm pressure, substance X will have the higher boiling point

The vapor pressure of liquid SO, is 281.1 mmHg at a temperature of 242.0 K. The enthalpy of vaporization, AH, What is the vapor pressure of SO2 at a temperature of 250.0 K, in mmHg? for this liquid is 24.9 kJ/mol. чар"

Prior to the discovery that freon-12 (CF2Cl2) was harmful to the Earth's ozone layer, it was frequently used as the dispersing agent in spray cans for hair spray, etc. Its enthalpy of vaporization at its normal boiling point of -29.2 degree C is 20.25 kJ/mol. Estimate the pressure that a can of hair spray using freon-12 had to withstand at 40 degree C, the temperature of a can that has standing in sunlight.