2. Thermodynamics of growth and product formation. Starting with Equation 11.19, derive Equation 11.20 (case in which µ is very large). YDP = YDP = YD YP YD Yx YP max 1+ 1 Ym DX u+ max -H+(-m₂) YD (-m₂) Yp 1 Yx (AGcat/YD) YXG (11.20) (11.19)
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- P2 657°C Isothermal 2.0 atm 37°C 3 0+ V(L) V3 The figure (not to scale) shows a pV diagram for 3.4 g of helium gas (He) that undergoes the process 1 → 2 → 3→1. The ideal gas constant is R = 8.314 J/mol · K = 0.0821 L· atm/mol · K, and the atomic weight of helium is 4.0 g/mol. What is the net work done by the gas in Joules? Please give your numerical answer with one decimal place.2. Find the steady-state temperature distribution u in a solid semi-infinite cylinder of radius a if the boundary temperature are u = 0 u = y = rsind at r=1 & at z = 010.13 Show that for a gas obeying the van der Waals equation (P+ a/v²) (v – b) = RT, with cy a function of T only, an equation for an adiabatic process is T(v – b)R/cv = const.
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- 17.Use the Gibbs expression for entropy (eqn 14.48) to derive the formula for the entropy of mixing (eqn 14.40). Below are equations 14.48 and 14.40 - AS-NkB(x ln x + (1 − x) ln(1 - x)). = S = -kB Piln P¿. (14.40) (14.48)A sealed 73 m tank is filled with 8000 moles of ideal oxygen gas (diatomic) at an initial temperature of 270 K. The gas is heated to a final temperature of 390 K. The atomic mass of oxygen is 16.0 g/mol. The mass density of the oxygen gas, in Sl units, is closest to: O 7.0 O 4.4 O 2.6 О 35 O 1.8
- 2.Consider a sample containing 1.60 mol of an ideal diatomic gas. (a) Assuming the molecules rotate but do not vibrate, find the total heat capacity of the sample at constant volume. nCv = ? (b) Assuming the molecules rotate but do not vibrate, find the total heat capacity of the sample at constant pressure.nCp = ? (c) Assuming the molecules both rotate and vibrate, find the total heat capacity of the sample at constant volume.nCv =? (d)Assuming the molecules both rotate and vibrate, find the total heat capacity of the sample at constant pressure.nCp = ?A process at constant volume pressure takes n mole vibrating diatomic from an initial temperature T to a final temperature 3T. Calculate the change in enthalpy, AH. Select one: O a. O b. ΔΗ AH = 9nRT AU = 5n RT O c. AH 11nRT ΔΗ O d. AH = 7nRT -2 mol of an ideal monoatomic gas moves from State 1 to State 2 P at constant pressure 1000 Pa and size V1=2 m3,V2 =3 m3. Calculated value W, Q, U, TI, T2