(1) The normal boiling point of argon is -189.35 °C at 1.00 atm and its heat of vaporization value is 1.210 kJ/mol. Calculate the pressure of argon when the temperature is changed to 0.00 °C. Express the final pressure of Ar in pounds per square inch (psi) units.

Follow the step-wise process outlined in Problem 31 to calculate the amount of heat involved in condensing 100.00 g of benzene gas (C6H6) at 80.00C to liquid benzene at 25.00C. Use Tables 8.1 and 8.2 for the specific heat, boiling point, and heat of vaporization of benzene.

The vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.

Is it possible to liquefy nitrogen at room temperature (about 25 C)? Is it possible to liquefy sulfur dioxide at room temperature? Explain your answers.

A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their properties, since one is a molecular solid and the other is an ionic solid. How do the properties differ and why?

When I mole of benzene is vaporized at a constant pressure of 1.00 atm and at its boiling point of 353.0 K, 30.79 kJ of energy (heat) is absorbed and the volume change is +28.90 L. What are E and H for this process?

Consider two different organic compounds, each with the formula C2H6O. One of these compounds is a liquid at room conditions and the other is a gas. Write Lewis structures consistent with this observation, and explain your answer. (Hint: The oxygen atom in both structures satisfies the octet rule with two bonds and two lone pairs.)

Why do the boiling points of the noble gases increase in the order HeNeArKrXe?

Helium condenses to a liquid at 4.224 K under atmospheric pressure and remains a liquid down to the absolute zero of temperature. (It is used as a coolant to reach very low temperatures.) The vapor pressure of liquidhelium at 2.20 K is 0.05256 atm. Calculate the volume occupied by 1.000 mol helium vapor under these conditions and compare it with the volume of the same amount of helium at standard temperature and pressure.

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