Thank you,, happy to help you,, have a very good day,, please like
The internal energy, U, is the total energy of a system. For any isolated system, the...
The correct answer does not depend on K or V. - Part A - The dependence of U on V Given the relationship (%), =T(E), -P, use the cyclic rule to write (@uſav), in terms of the measurable quantities P, B, T, and K. Recall that B and k are the isobaric volumetric thermal expansion coefficient and the isothermal compressibility, respectively, defined by B= + () and k=-* (*) Express your answer in terms of P,B, T, and K. ►...
12) we also show in Lecture #5 that, for any system, OU where β is the constant-pressure (isobaric) thermal expansivity and κ is the constant temperature (isothermal) compressibility. Use this result, along with typical values for /P and K, to show that it is a good approximation to neglect the dependence on volume of the internal energy ofa liquid or solid. Explicity, show that: TF
2. Consider free expansion of a gas when the internal energy U remains constant. Derive: a) the expression for (дт/avJu in terms of P, T, Cv and (ap/aT)v b) the expression for (as/aV)u in terms of P and T c) using equations obtained in a) and b) calculate (expression for) the change of temperature AT and change of entropy AS for a free gas expansion from Vi to V2. 2. Consider free expansion of a gas when the internal energy...
(a) One mole of a monoatomic van der Waals gas obeys the equation of state A3. ) (V-b)=RT (p+ and its internal energy is expressed as U CvT where Cv is the molar isochoric heat capacity of an ideal gas. The gas is initially at pressure p and volume V (i) Explain the physical meaning of the parameters a and b in the equation of state of the gas (ii) Write down the equation that defines entropy in thermodynamics. Define...
What is the sign of AU as the system of ideal gas goes from point A to point B on the graph? (Hint the U is function of temperature only for a perfect gas) P (atm) 5 4 3 2 В 1 V (m3) 2 5 1 4 The states And B have the same internal energy, so delta U is zero The internal energy of the system increases, so delta U is positive The internal energy of the system...
2. Find the changes in internal energy (AU) and enthalpy (AH) per kmol, for air going from 10 bar, 277 K and 2.28 m3/kmol (molar volume), to 333 K and 1 atm. Use the following: 4 Cp = 29.3 kJ kmol-? K-1 Cy = 21 kJ kmol-? K-1 PV/T = constant Do not use any additional properties of ideal gases. There is no need to prove the gas is ideal or to use such properties. Hint: split the process up...
The multiplicity of a system of N quantum oscillators with the total internal energy U and energy quantum a is Ω(,- ,N) = and q 1 and use Stirling's approximation, N(N), to derive U (T, N). You can replace N-1 with N in multiplicity equation to simplify writing given that N1 (N-1+9)!. Assume that both N » 1
An isolated system contains an ideal gas with state parameters: U, T, S, P, V, M, N. (vii) (viii) Describe an irreversible process that increases both the internal energy of the system, U, and the entropy of the system, S. Calculate the increase in entropy that results from the process you have chosen. What is the source of the increase entropy in this process? (ix)
Please also explain the difference between delta H and delta U. Thanks! 2. Find the changes in internal energy (AU) and enthalpy (AH) per kmol, for air going from 10 bar, 277 K and 2.28 m3/kmol (molar volume), to 333 K and 1 atm. Use the following: 4 Cp = 29.3 kJ kmol-? K-1 Cy = 21 kJ kmol-? K-1 PV/T = constant Do not use any additional properties of ideal gases. There is no need to prove the gas...
02) Consider a hydrostatic system represented by the thermodynamic variables volume V, pressure P and temperature T. a) Consider entropy S = S(T, V) and derive the equation TdS. Tas = Cvat +T (1) dV. V Show that this equation can be written as follows BT TdS = CydT + PDV where Cv is the thermal capacity at constant volume, B is the isobaric expansiveness and K is isothermal compressibility: b) Consider a gas described by the equation of state...