# Physical Chemistry PDF

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answer the problems in the PDF file attached and allow add explanations and brief summary how you answer the problem so I could understand what going on

CHMY 373 2019 – Problem Set 2 Due: Friday Jan. 25 Reminder: See previous problem set and/or the syllabus for rules regarding problem sets. Reading: Chapter 19.1‐19.5, Simon & McQuarrie 1. Reversible compression: a reversible process is a thought experiment where every infinitesimal step of the process represents an equilibrium state. Consider the reversible compression of 1.0 mole of an ideal gas from 22 L to 2.2 L, at a constant temperature of 25 °C. a. Draw a schematic for and describe an experimental setup that would imitate a reversible compression at constant temperature. b. Determine the work, heat, and for this process, in units of kJ. 2. Irreversible compression: one type of irreversible process is a constant pressure compression or expansion. Consider the constant pressure compression of 1.0 mole of an ideal gas from 22 L to 2.2 L, at a constant temperature of 25 °C. a. In the faded instruction manual for this process, it says the process should be carried out at a constant pressure of either 15 bar or 1.5 bar. Which value must it be? Hint: one of the two options is impossible to carry out b. Determine the work, heat, and for this process, in units of kJ. 3. Chemical reactions can result in work being performed on the environment. Consider the initial state of a system as follows: 12 g of CaCO3 s lie in a container fitted with a piston constrained by a fixed external pressure. For the purposes of this problem, consider the initial volume of the container to be negligible consider all solids to have a negligible volume . The container is then heated to 1000 °C. During heating, the sample completely decomposes to CaO s and CO2 g at a temperature of 760 °C. a. Calculate the work in kJ for the complete process arising from the mechanical expansion of the system against a fixed external pressure corresponding to ambient pressure in Bozeman 0.85 bar , assuming that the gas released is ideal. b. Do you expect the work to be higher or lower if the CO2 released is “real CO2” and therefore has a slightly higher volume than an ideal gas at the end of the process i.e., its compressibility factor, , is greater than 1 at 1000 °C ? 4. The so‐called “ ” of a fluid or material is a measure of the intermolecular forces within it, and is defined by: , , Derive an expression for the internal pressure of: a. an ideal gas. b. a van der Waals gas. c. a Berthelot gas, defined by: d. a Dietericci gas, defined by: 5. Reversible vs. Free. Consider the expansion of a system containing pure oxygen gas, which can be fairly accurately described by the van der Waals equation of state see Table 16.3 for accurate vdW constants . Assume that the molar isochoric heat of oxygen is 5/2 and is therefore independent of T. capacity a. Determine the final temperature, , when 1.0 mole of oxygen undergoes a reversible adiabatic expansion from 1.0 L to 24 L, if it is initially at 298 K. b. Determine the final temperature, , when 1.0 mole of oxygen undergoes a free adiabatic expansion from 1.0 L to 24 L, initially at 298 K. c. Describe the qualitative relationship between the heat, work, and of these two processes i.e., greater than, less than, or equal .

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Anonymous
Good stuff. Would use again.

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