An Introduction to Thermal Physics
1st Edition
ISBN: 9780201380279
Author: Daniel V. Schroeder
Publisher: Addison Wesley
expand_more
expand_more
format_list_bulleted
Question
Chapter 2.6, Problem 34P
To determine
To Prove:The change in entropy in quasistatic isothermal expansion of monoatomic ideal gas is related to the input heat.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Show that during the quasistatic isothermal expansion of a monatomic ideal gas, the change in entropy is related to the heat input Q by the simple formula.
SΔ= Q/TIn the following chapter I'll prove that this formula is valid for any quasistatic process. Show, however, that it is not valid for the free expansion process described above.
By considering the number of accessible states for an ideal two-dimensional gas made up of N adsorbed molecules on a surface of area A, obtain an expression for the entropy of a system of this kind. Use the entropy expression to obtain the equation of state in terms of N, A, and the force per unit length F. What is the specific heat of the two-dimensional gas at constant area?
Hi, could I get some help with this macro-connection physics problem involving isothermal expansion?
The set up is:
For an isothermal reversible expansion of two moles of an ideal gas, what is the entropy change of the a) gas and b) the surroundings in J/K to 4 digits of precision if the gas volume quadruples, assuming NA = 6.022e23 and kB = 1.38e-23 J/K?
Thank you.
Chapter 2 Solutions
An Introduction to Thermal Physics
Ch. 2.1 - Prob. 1PCh. 2.1 - Prob. 2PCh. 2.1 - Prob. 3PCh. 2.1 - Prob. 4PCh. 2.2 - For an Einstein solid with each of the following...Ch. 2.2 - Prob. 6PCh. 2.2 - Prob. 7PCh. 2.3 - Prob. 8PCh. 2.3 - Use a computer to reproduce the table and graph in...Ch. 2.3 - Use a computer to produce a table and graph, like...
Ch. 2.3 - Use a computer to produce a table and graph, like...Ch. 2.4 - Prob. 12PCh. 2.4 - Fun with logarithms. (a) Simplify the expression...Ch. 2.4 - Write e1023 in the form 10x, for some x.Ch. 2.4 - Prob. 15PCh. 2.4 - Prob. 16PCh. 2.4 - Prob. 17PCh. 2.4 - Prob. 18PCh. 2.4 - Prob. 19PCh. 2.4 - Suppose you were to shrink Figure 2.7 until the...Ch. 2.4 - Prob. 21PCh. 2.4 - Prob. 22PCh. 2.4 - Prob. 23PCh. 2.4 - Prob. 24PCh. 2.4 - Prob. 25PCh. 2.5 - Prob. 26PCh. 2.5 - Prob. 27PCh. 2.6 - How many possible arrangements are there for a...Ch. 2.6 - Consider a system of two Einstein solids, with...Ch. 2.6 - Prob. 30PCh. 2.6 - Fill in the algebraic steps to derive the...Ch. 2.6 - Prob. 32PCh. 2.6 - Use the Sackur-Tetrode equation to calculate the...Ch. 2.6 - Prob. 34PCh. 2.6 - According to the Sackur-Tetrode equation, the...Ch. 2.6 - For either a monatomic ideal gas or a...Ch. 2.6 - Using the Same method as in the text, calculate...Ch. 2.6 - Prob. 38PCh. 2.6 - Compute the entropy of a mole of helium at room...Ch. 2.6 - For each of the following irreversible process,...Ch. 2.6 - Describe a few of your favorite, and least...Ch. 2.6 - A black hole is a region of space where gravity is...
Knowledge Booster
Similar questions
- A copper rod of cross-sectional area 5.0 cm2 and length 5.0 m conducts heat from a heat reservoir at 373 K to one at 273 K. What is the time rate of change of the universe's entropy for this process?arrow_forwardTwo hundred grams of water at 0 is brought into contact into thermal equilibrium successively with reservoirs at 20 , 40 , 60 , and 80 . (a) What is the entropy change of the water? (b) Of the reservoir? (c) What is the entropy change of the universe?arrow_forwardA cylinder contains 500 g of helium at 120 atm and 20 . The valve is leaky, and all the gas slowly escapes isothermally into the atmosphere. Use the results of the preceding problem to determine the resulting change in entropy of the universe.arrow_forward
- In a living cell, which is an open system that exchanges energy and matter with the exterior, the entropy can decrease, i.e. dS < 0. Explain how this is possible in terms of de S and di S. How is the Second Law valid in this case?arrow_forwardA mass m of water is heated reversibly from temperature T to T, at a constant pressure of P. In this problem, we are going to determine an expression for the change in entropy, AS. Assume we can heat the given water infinitesimally slowly so that the process is reversible. Therefore, heat in any infinitesimal step is given by the following: dQ = mc dT, where c is the specific heat and is constant. Calculate the change in entropy in cal/K for a sample of water with mass m= 1.6 kg and changing temperature from T1 = 24.2°C to T2= (24.2+10)°C. The specific heat c of water is 1,000 cal/kg/K. AS=arrow_forwardFor one component gas that is confined in a box with volume V. V We can get the entropy of the gas as S = Nk, In where N is the total number of atoms, a is the radius of the atom. Can you guess (or work out) how it is obtained?arrow_forward
- Consider a system with a certain energy content, from which we wish to extract as much work as possible. Should the system’s entropy be high or low? Is this orderly or disorderly? Structured or uniform? Explain briefly.arrow_forwardA monatomic ideal gas initially has a temperature of 330k and preassure of 3x105 Pa. The gas expands from a volume of 500cm3 to a volume of 1500cm3. Calculate the work done by the gas (in Joules) if the expansion is isothermal. Calculate the change in internal energy (in Joules), if the expansion is adiabatic. I know that the first two questions have the same results, but, why the work equals the change in internal energy? I know that in adiabatic expansion the work done equals the change in internal energy(which is negative). To calculate the work I could use the same formula as the first question, so, is that the reason for they to be equal? I was trying to calculate the result for the last question using the formula Δu = g/2*n*r*Δt, so, how can I find the change in internal energy considering this fomula and get to the same result?arrow_forwardFind the final temperature when 50 kg of water at 20 °C and 100 kg of water at 26 °C are mixed. Neglect heat loss to the surroundings. Hence calculate the net change in Entropy for this process. Integrate to get AS, do NOT estimate.arrow_forward
- A mass m of water is heated reversibly from temperature T1 to T2 at a constant pressure of P. In this problem, we are going to determine an expression for the change in entropy, ΔS.Assume we can heat the given water infinitesimally slowly so that the process is reversible. Therefore, heat in any infinitesimal step is given by the following: dQ = mc dT, where c is the specific heat and is constant. Part (a) Write an expression for the change in entropy ΔS for the system. Part (b) Calculate the change in entropy in cal/K for a sample of water with mass m = 1.9 kg and changing temperature from T1 = 22.9°C to T2 = (22.9+10)°C. The specific heat c of water is 1,000 cal/kg/K.arrow_forwardIn order to take a nice warm bath, you mix 50 liters of hot water at 55°C with 25 liters of cold water at 10°C. How much new entropy have you created by mixing the water? Can you please help me with this problem show a complete and explicit solution with an explanation step by step. Note: No shortcuts and don't skip any mathematical algebra.arrow_forwardA certain Carnot engine operates between 290 K and 450 K. The engine does 150 J of work for every 600 J of heat absorbed from the combustion of fuel. Find the actual efficiency and the theoretical efficiency. Find the heat exhausted to the cold reservoir. Find the entropy change of the hot reservoir and the cold reservoir, and the net change of entropy of the entire engine. (For this finding the change in entropy, Qh is negative as energy is leaving the reservoir, Qc is positive)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
