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This paper contains hints and answers for solving practice final a. When I provide a hint, There is often one simple step to go from that hint to the...

Can you help me solve these problems. The "solutions by steps" is what I'm looking for, not so much the answers. File is attached with the answer key.

This paper contains hints and answers for solving practice final a. When I provide a hint, There is often one simple step to go from that hint to the final solution. If you are unable to use the hint to obtain the final solution, make sure to attend an office hour or read the book to understand why! If I put “…” it means that the answer should be readily apparent from the problem. If not, you should ask during office hours how it is apparent! (don’t just ask for the answer, it wont help you!). (I don’t know if all these answers are correct, but I think they are). I’m not providing straight solutions, because I want you guys to work these problems out so you can be successful on the final. If I sound demeaning on some of the hints, that’s not my intention! Rather, my intention is to point out how some answers are very simple (and that many times as a student you make it more difficult than it needs to be!). Problem 1. a)Ti=36.1K Tb=12K. b) deltaU(i->a) (isothermal process…) deltaU(a->b) 1000J (is this positive or negative….) c) …. d)For this problem…. Use the answers you got in b to make it easy! Q(i->a) (isothermal process) Q(a->b) (W=400… deltaU=Q+W) e) should this be positive or negative…. Problem 2. a) read the question for this answer b) Eth of ice changes Eb of water changes c) 82kJ d) draw a phase-diagram if you’re confused about this. When does the water stop supplying heat to the ice? e) we solved for Q already, what is Tave? Just plug them in… Think… should the entropy of the ice be going up or down? f) Same a above… we know how much Q left the water… we know the temperature. g) should the total S be positive or negative? As a ‘common sense’ check, In real life… if you place ice in water, will the ice come to thermal equilibrium with the water? Is this spontaneous then?
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Problem 3. a) mgh b) deltaPE+deltaKE=0 c)…(did any energies change between the bottom of the slope, and the point directly before the spring?) d) deltaKE+deltaPE(m-s) = 0 e) now…. KE(new) = KE(old) – 30J. then redo previous problem with KE(new)… deltaKE(new)+deltaPE(m-s) = 0 Should it compress more or less? Problem 4. a) What is Eth at 0K? Ebond = number of bonds*bond energy. (how many bonds are there in a 3D close-packed solid? If you have Na atoms… do you divide this number by 2? Think about why you might divide by 2). Etot = Ebond + Eth. b) distance is r0. How is this related to sigma? a) you add energy…. How is this energy split between Eth and Ebond. b) use answer to above question to get numbers. (add new energy to original Ebond and Eth you got in first part a) c) I don’t like this question… you can think that each atom gets 3epsilon of energy… so each bond (since there are 12), gets epsilon/4 of this energy…. . but… it actually gets double this since the other atom in the bond also adds epsilon/4 energy to this bond. (atleast, I think that’s correct). Don’t worry about this problem though. Problem 5. a) … b)cv=deltaU/deltaT c) cv/mole = #modes/2*R d) … e) huh? I don’t see how this is different from d…. it looks like a backwards d to me… let me know if you understand what this question wants! Problem 6. a) first find the Q necessary to freeze the water. Recognize that this Q leaves the water and enters the room. Then use deltas=Q/Tave to find the change in entropy of the water,
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Quiz practice fnal DL Sec Grading: Last 6 digits oF student ID: Name: ±irst three letters oF your Family name 1. . Consider the process shown on the PV diagram to the right. In this process, two moles of a di- atomic ideal gas perform a loop from the initial state i through two intermediate states a, b , back to the initial state. The step connecting i to a is an isothermal process. (a) Find the temperature for each state (i.e. i, a, b ) along the process. (b) Find the change in internal energy of the system for each one of the three steps along the loop. (c) Find the total change in internal energy of the system. (d) Knowing that along the isothermal process the work is - 659 J , ±nd the amount of heat for each step of the loop and the total amount of heat. (e) Find the total work along the loop.
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2. A 2 kg block of ice initially at T = - 20 C is put in contact with a very large amount of liquid water at T = 0 C (by “very large amount” we imply that by the time ice and water reach thermal equilibrium, there will still be some liquid water left). Ice and water can exchange heat just with each other but not with the environment. The speciFc heat of water is 4186 J kg · K and of ice is 2050 J kg · K . (a) What is the Fnal equilibrium temperature of the system? (b) Draw a complete energy system diagram for the process, clearly showing all the indicators for initial and Fnal state. (c) ±ind the amount of heat absorbed by the ice in the process. (d) ±ind the Fnal mass of ice in the system at equilibrium (e) ±ind the the change in entropy of the 2 kg -block of ice. (f) ±ind the the change in entropy of the very large amount of water. (g) By Fnding the total change in entropy, determine if the process is spontaneous or not.
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Hi! I have added diagram For... View the full answer


1. a) It is given that the path from initial to state “a” is isothermal. This means that
temperature remains constant.
For initial state:
Pi= 6*10^5 Pa =6* 0.987atm
Vi = 10^-3 mL = 1L

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