19.A sample consisting of 1 mol diatomic gas molecules at 200 K is compressed reversibly and adiabatically until its temperature reaches 250 K. Given Cym = 27.5 J K-1 mol-1, calculate Q, W, AU, AH, AS.
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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.Calculate the molar entropy of an ensemble by S=U/T+klnQ with 1.32 mole of Kr(g) at 47degree and a pressure of 1.7 bar.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).
- Calculate the molar heat capacity at constant pressure (Cp) for a diatomic H2 gas(y = 1.41) with molar heat capacity at constant volume (Cv) of 20.42 J/mol-K?calculate the final temperature of a sample of carbon dioxide of mass 16.0g that is expanded reversibly and adiabatically from 500cm3 at 298.15K to 2dm3 if Cp,m is equal 37.11J/K.mol.Hydrogen is one of only seven elements which exist as stable diatomic molecules at (or close to) room temperature and atmospheric pressure. Let’s investigate just how much more thermodynamically favorable diatomic hydrogen is compared to atomic hydrogen. Given the following reaction and associated data at T = 298.15 K. 2 H(g) ⇌ H"(g) or equivalently H(g) + H(g) ⇌ H2(g) Δf?° (kJ mol-1) ?° (kJ K-1 mol-1) H(g) 218.0 0.115 H2(g) 0 0.131 Calculate ΔH, ΔS, and ΔG for the formation of H2(g) from H(g) at 298.15 K. Calculate KP for the reaction. Calculate the temperature at which the reverse reaction becomes favorable. Assume ΔH and ΔS do not change with temperature.
- The constant-pressure heat capacity of a sample of a perfect gas was found to vary with temperature according to the expression Cp(JK–1) = 20.17 + 0.03665(T). Calculate q, w, ΔU, and ΔH when the temperature is raised from 25°C to 300°C(a) at constant pressure(b) at constant volumecalculate the standard molar entropy of neon gase at 200K and 298.15KQI/Calculate the AS, AE, AH,q.W for a hundredfold isothermal reversible at 25°C of a mole of perfect gas.
- Calculate the contribution that rotational motion makes to the molar entropy of a gas of HCl molecules at 25 °C.One mole of a monatomic ideal gas begins in a state withP 5 1.00 atm and T 5 300 K. It is expanded reversiblyand adiabatically until the volume has doubled; then it isexpanded irreversibly and isothermally into a vacuumuntil the volume has doubled again; and then it is heatedreversibly at constant volume to 400 K. Finally, it is compressed reversibly and isothermally until a inal state withP 5 1.00 atm and T 5 400 K is reached. Calculate DSsysfor this process. (Hint: There are two ways to solve thisproblem—an easy way and a hard way.)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