Show that the statistical definition of the internal energy (U = E, E,p;) and the entropy (S = -k E;p; In(e;)), where (p;) is the Boltzmann distribution, are consistent with the differential form of the fundamental equation of thermodynamics (dU = T'dS - PdV).
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- The constant-pressure heat capacity of a sample of a perfect gaswas found to vary with temperature according to the expression Cp/(J K−1) = 20.17 + 0.3665(T/K). Calculate q, w, ΔU, and ΔH when the temperature is raised from 25 °C to 100 °C (i) at constant pressure, (ii) at constant volume.Predict the output of energy as heat from the combustion of 1.0 dm3 of octane at 298 K and 1 bar. Its mass density is 0.703 g cm−3 ?When 3.0 mol O2 is heated at a constant pressure of 3.25 atm, itstemperature increases from 260 K to 285 K. Given that the molar heatcapacity of O2 at constant pressure is 29.4 J K−1 mol−1, calculate q, ΔH,and ΔU.
- Without carrying out an explicit calculation, explain there lative values of the standard molar entropies (at 298 K) of the following substances: (a) Ne(g) (146 J K-1 mol-1) compared with Xe(g) (170 J K-1 mol-1), (b) H2O(g) (189 J K-1 mol-1) compared with D2O(g) (198 J K-1 mol-1), (c) C(diamond) (2.4 J K-1 mol-1) compared with C(g raphite) (5.7 J K-1 mol-1).dU = Cv dT + PT dV where Cv is the constant volume heat capacity and PT is the internal pressure. (a) Derive (∂V/∂T )_U in terms of Cv and/or PT. (b) If the molecules in the system are interacting through repulsive forces, then determine the sign PT of and (∂V/∂T )_U. Namely choose the sign: PT (<, = , >) 0 and (∂V/∂T )_U (<, = , >) = 0.2. The energy levels of a CH3-group attached to a larger fragment are given by the expression for a particle on a ring, provided the group is rotating freely. The moment of inertia for the rotation isI = 5.341 x 10-47 kgm2. What is the associated heat capacity (Cv) at 298 K? What is the associated entropy at the same temperature?
- The molar heat capacity of N2(g) in the range 200K to 400K is given by Cpm (J/Kmol)= 28.58+3.77*10^-3 (T/K). Given that the standard molar entropy of N2(g) at 298K is 191.6 J/Kmol, determine q, w, change in enthalpy (H), change in internal energy (U), and change of entropy of the system (Ssys) when the temperature is raised from 25C to 100C under a) constant pressure and b) constant volume.A sample of carbon dioxide that initially occupies 15.0 dm3 at 250 K and 1.00 atm is compressed isothermally. Into what volume must the gas be compressed to reduce its entropy by 10.0 J K-1?calculate the standard molar entropy of neon gase at 200K and 298.15K
- Calculate the change in the entropies of the system and the surroundings, and the total change in entropy, when the volume of a sample of argon gas of mass 21 g at 298 K and 1.50 bar increases from 1.20 dm3 to 4.60 dm3in (a) an isothermal reversible expansion, (b) an isothermal irreversible expansion against pex = 0, and (c) an adiabatic reversible expansion.Determine the entropy of reaction at T= 298.15K and standard pressure.A sample of K(s) of mass 3.226 gg undergoes combustion in a constant volume calorimeter at 298.15 K. The calorimeter constant is 1849 J⋅K−Mol-, and the measured temperature rise in the inner water bath containing 1538 gg of water is 1.776 K. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1CP,m(H2O,l)=75.3J⋅mol−1⋅K−1. 1) Calculate ΔU���f for K2O 2) Calculate ΔH∘f for K2O