V Show that (35) = Cp/aTV to calculate the pressure in bar. Hint: use the equation sheet to find a helpful equation for ds and use the partial derivative sheet to find a helpful equation for a.
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- Q-1: A mixture of ideal gases possesses the properties listed in table below when examined at 2 bar and 22°C giving the following gravimetric analysis. A: 20% ; B: 25% ; C: 30% ; D 25% Find for the mixture: Volumetric analysis. Gas constant. • Enthalpy. • Partial pressure for each constituent Gas A B C M Kg/kmol 18 14 46 28 kJ/kmol K 20.6 16.7 24.2 21.33-28 A 1.8-m3 rigid tank contains steam at 220°C. One-third of the volume is in the liquid phase and the rest is in the vapor form. Determine (a) the pressure of the steam, (b) the quality of the saturated mixture, and (c) the density of the mixture. Value (5/30) Steam 1.8 m 220°CData: INCLUDE UNITS!!! Barometric Pressure: A B C D E F G H 1 J K L M N Calculations: INCLUDE UNITS AND SHOW WORK (attach scratch paper or use back side of the page)!!! Trial 1 Trial 2 Trial 3 0 P 2 H,0,(aq) 759 forr Mass of 10 mL grad cylinder with ~5 mL H₂O: solution Mass of empty 10 mL grad cylinder Initial gas volume reading Final gas volume reading Q Temperature (°C) Vapor pressure of water (from Table 8-1) Mass of H₂O₂ solution used Volume of gas collected, in ml Volume of gas collected, in L Partial pressure of Oz, in torr Partial pressure of O₂, in atm Temperature (K) Number of moles of Oz formed Number of moles of H₂O₂ consumed Mass of H₂O2 consumed (molar mass = 34.02 g/mol) Mass percent H₂0₂ in solution KI (cat.) Average mass % H₂O₂ 15 16 17 18 19 20 21 22 23 2 H₂0 (aq) + O₂(g) Trial 1 Trial 2 50.081 49-838 45.392 45.383 50ml. 59 mal 22.4°C 22.4°C 17.5 18.6 19.8 21.1 8-7 Temperature (°C) Vapor Pressure (torr) Temperature (°C) 12.8 13.6 14.5 15.5 16.5 PBaR=75968! Trial 3…
- Starting from the definition of Cp and Cv, derive the expression of (C₁-Cv) expressed only in measurable quantities.1. A perfect gas undergoes compression at constant temperature, which reduces its volumeby 3.08 dm3. The final pressure and volume of the gas are 6.42 bar and 5.38 dm3, respectively. Calculate the original pressure of the gas in (a) bar, (b) atm. 2. Consider an isothermal column of an ideal gas at 25oC. What must be the molar mass ofthis gas be if the pressure is 0.80 of its ground level value at (a) 10km and (b) 1km ? Please show complete solutionsA gas mixture consists of 0.62 percent N, and 0.38 percent CO, by mole basis. Take 1 kg mole of the mixture and the molecular weight of N2 and CO2 are 28 and 44 kg/kg.mol respectively. Determine the (i) mole fractions of the constituents, (ii) mass fractions of constituents, (ii) the average molar mass of the mixture, and (iv) the average gas constant of the mixture. Take universal gas constant is 8.314 kJ/k mole.K. mole fraction of N2 mole fraction of CO2 Mass fraction of N2 Mass fraction of CO2 Molar Mixture Mixture gas constant
- E, In k =- +In A RT If this equation is in the slope-intercept form of a line, which term in this equation corresponds to: R is the thermodynamic gas constant (8.31 x 10-3 kJ/K mol). у? In K x? 1/T m? -Ea/r b? In A c-f)I Record the equation of the trendline below. Attach your table of values for the calculated data and your linear plot in your assignment. Equation: у%3D102х + 1.6 R2 = 0.95 g) Using the equation of the best-fit line determine i) and ii) (see below). Show your complete work in the space provided. i) the value of E (in kJ/mol) Click here to enter text. ii) the value of A (in s-) Click here to enter text. nFocusCp is greater than or equal to Cv. Why?A sample of blood plasma occupies 0.550 dm3 at 0 ocand 1.03 bar, and is compressed isothermally by 0.57 per
- In this week's last lecture, we showed you can use the Maxwell relationship as as (²²),= (-), * to derive and expression for an ideal gas where (35) = nR/V = R/Vm as Following this same logic, derive the expression for (5) using the van der Waals equation of state to substitute for pressure (hint: best to use the form of the EOS that uses molar volume Vm)(1) The relationship between C P.m and C V.m can also be given by the relationship: CP.m - Cym = T| aT (a) Use the above equation to demonstrate that C P.m - C V.m - R for an ideal gas. (b) Demonstrate the expression C P.m - C V.m for a gas obeying the equation of state: PVm = RT + B(T)PA mixture of ideal gases possesses the properties listed in table below when examined at 2 bar and 22 C giving the following gravimetric analysis. A: 20% ; B: 25% ; C: 30%; D 25% Find for the mixture: • Volumetric analysis. • Gas constant. • Enthalpy. Partial pressure for each constituent Gas A Kg/kmol 28 16.7 24.2 21.3 M 18 14 46 C, kJ/kmol K 20.6