물리화학 대학교재솔루션 (Physical Chemistry for the Life Sciences (Paperback) , Thomas Engel 저) 자료

물리화학 대학교재솔루션 (Physical Chemistry for the Life Sciences (Paperback) , Thomas Engel 저) 자료

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물리화학 대학교재솔루션 (Physical Chemistry for the Life Sciences (Paperback) , Thomas Engel 저)

[솔루션] 물리화학 솔루션 (Physical Chemistry for the Life Sciences(Paperback), Thomas Engel 저) 입니다. 총 1장부터 19장까지 구성되어 있습니다..^^ 공부하는 저로써는.. 공부 할 때 정말 도움이 많이 됬던 자료 입니다. 수업을 따라가면서 이해 안가는 부분이 있으면 체크 하는 방식도 괜찮으며, 또 수업이 들은지 오래되어 다시 공부하고자 할때 도움이 되는 솔루션입니다..^^ 그리고 시험기간에는 정말 없어서는 안될 자료이기도 하구요..^^

총 1장부터 19장까지 구성되어 있습니다.


1장의 솔루션 일부를 발췌했습니다. (수식이은 게시판에 호환되지 않으니 양해 바랍니다..^^)


Chapter 1: Fundamental Concepts of Thermodynamics
Problem numbers in italics indicate that the solution is included in the Students Solutions Manual.
Questions on Concepts

Q1.1) The location of the boundary between the system and the surroundings is a choice that must be made by the thermodynamicist. Consider a beaker of boiling water in an airtight room. Is the system open or closed if you place the boundary just outside the liquid water? Is the system open or closed if you place the boundary just inside the walls of the room?

If the system boundaries are just outside of the liquid water, the system is open because water can escape from the top surface. The system is closed if the boundary is just inside the walls, because the room is airtight.

Q1.2) Real walls are never totally adiabatic. Order the following walls in increasing order with respect to being diathermal: 1-cm-thick concrete, 1-cm-thick vacuum, 1-cm-thick copper, 1-cm-thick cork.

1-cm-thick vacuum < 1-cm-thick cork < 1-cm-thick concrete < 1-cm-thick copper

Q1.3) Why is the possibility of exchange of matter or energy appropriate to the variable of interest a necessary condition for equilibrium between two systems?

Equilibrium is a dynamic process in which the rates of two opposing processes are equal. However, if the rate in each direction is zero, no exchange is possible, and therefore the system can not reach equilibrium.

Q1.4) At sufficiently high temperatures, the van der Waals equation has the form . Note that the attractive part of the potential has no influence in this expression. Justify this behavior using the potential energy diagram in Figure 1.6.

At high temperatures, the energy of the molecule is large as indicated by the colored rectangular area in the figure below.

In this case, the well depth is a small fraction of the total energy. Therefore, the particle is unaffected by the attractive part of the potential.

Q1.5) The parameter a in the van der Waals equation is greater for H2O than for He. What does this say about the form of the potential function in Figure 1.6 for the two gases?

It says that the depth of the attractive potential is greater for H2O than for He.

Problems

P1.1) A sealed flask with a capacity of 1.00 dm3 contains 5.00 g of ethane. The flask is so weak that it will burst if the pressure exceeds 1.00 × 106 Pa. At what temperature will the pressure of the gas exceed the bursting temperature?


P1.2) Consider a gas mixture in a 2.00-dm3 flask at 27.0ºC. For each of the following mixtures, calculate the partial pressure of each gas, the total pressure, and the composition of the mixture in mole percent.
a) 1.00 g H2 and 1.00 g O2
b) 1.00 g N2 and 1.00 g O2
c) 1.00 g CH4 and 1.00 g NH3

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