1. The triple point of acetone is at -94.5°C and 0.018 torr. Assume the molar heat of vaporization is 35.0 kJ/mol. a) Estimate the vapor pressure of acetone at -78°C (the temperature of a dry ice - acetone bath). b) Use the data given above to estimate the normal boiling point of acetone. c) What approximations have been made in your answers?

42. Determine the normal boiling point of a substance whose vapor pressure is 75.1 mm Hg at 35°Cand has a Hvap of 32.1 kJ/mol.

.  The vapor pressure and enthalpy of vaporization of an unknown substance are measured to be 479.6 torr and 35.3 kJ/mol, respectively at room temperature (298.15 K). Estimate the normal boiling point of the substance at an atmospheric pressure of 760 torr.

Use the References to access important values if needed for this question. The normal boiling point of liquid pentane is 309 K. Assuming that its molar heat of vaporization is constant at 26.8 kJ/mol, the boiling point of C5H12 when the external pressure is 1.23 atm is K.

O ADVANCED MATERIAL Using a phase diagram to predict phase at a given temperature... Study t. lowing phase diagram of Substance X. 0.4 solid liquid 0.2 gas 0. 200 400 temperature (K) Use this diagram to answer the following questions. Suppose a small sample of pure X is held at 166. °C and 0.2 atm. What will be the state of the sample? (choose one) 8 Suppose the temperature is held constant at 166. °C but the pressure is decreased by 0.1 atm. what will happen to the sample? (choose one) Suppose, on the other hand, the pressure is held constant at 0.2 atm but the temperature is decreased by 144. °C. What will happen to the v (choose one) sample? Nothing. It will melt. It will freeze. Explanation Check It will boil. It will condense. 20 80 F2 F3 F4 F5 pressure (atm) II

Below is the phase diagram for iodine. If you start with a sample of iodine at 150°C and 1.0 atm and you increase the temperature, what phase change will you observe? a. boiling b. melting c. sublimation d. melting, then boiling

The enthalpy of vaporization of Substance x is 7.00 kJ/mol and its normal boiling point is -10c . Calculate the vapor pressure of x at -36c. Round your answer to 2 significant digits

The enthalpy of vaporization for acetone is 32.0 kj/mol. the normal boiling point (at 1.00 atm) for acetone is 56.5 C. What is the temperature of acetone at 560 torr?

Water has a vapor pressure of 23.8 mm Hg at 25°C and a heat of vaporization of 40.657 kJ/mol. Using the Clausius-Clapeyron equation given below, determine the vapor pressure of water at 96°C.