2) Calculate the molar volume of a gas mixture containing 40 mole % NH3, 30% CO2 and 30 mole % C2H4, at a pressure of 300 atm and a temperature of 200°C, using the methods described below: (i) (ii) (iii) (iv) Ideal gas law Amagat's law and the rule of corresponding states Kay's rule and the rule of corresponding states Van der Waals equation of state and averaged constants

2) Calculate the molar volume of a gas mixture containing 40 mole % NH3, 30% CO2 and 30 mole % C2H4, at a pressure of 300 atm and a temperature of 200°C, using the methods described below: (i) (ii) (iii) (iv) Ideal gas law Amagat's law and the rule of corresponding states Kay's rule and the rule of corresponding states Van der Waals equation of state and averaged constants

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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 solutions
1. A rigid tank containing 1.36 kg gas mixture of nitrogen and carbon dioxide (each 50% by volume) at 272 kPa and 65°C. Determine (a) molar analysis (or % by mol (b) molecular weight and gas constant of mixture (c) volume of mixture (d ) partial volumes of gases (e ) partial pressures of gases (f) gravimetric analysis (or % by mass) (g ) masses of gases (h) mols of gases (i) specific heats Cp and Cv of mixture (j) specific heat ratio of mixture (k) internal energy of mixture (1) enthalpy of mixture Use subscripts: 1 = nitrogen (N,) 2 = carbon dioxide (CO,) no subscript = gas mixture From Table A-1 Specific Heats in kJ/kg K Cp, = 1.0414 Carbon dioxide Cp; = 0.8452 Nitrogen %3D %3D
(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)P
7A A mass m of a perfect gas [C=0.815 KJ/Kg K , cp=1.42 KJ/Kg K] is compressed from 0.85 m' and 105 N/m2 to volume 0. 034 m and pressure 3.0x10 N/m2 the temperature is reduced by AT = 100 K. the gas constant r in kJ/kgK. is
1.2(a) A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm. The final pressure and volume of the gas are 5.04 bar and 4.65 dm', respectively. Calculate the original pressure of the gas in (a) bar, (b) atm.
Underwater, the pressure increases by 1 bar for every 10 m of depth. When a scuba diver breathes pressurized air in which the partial pressure of N2(g) exceeds 4 bar, the result is nitrogen narcosis, which is similar to alcohol intoxication. What is the maximum mole percent of N2 in an air mixture that could be used by divers at depths up to 85 m below sea level without undue risk of nitrogen narcosis?
1.1 (a) A sample of air occupies 1.0 L at 25 °C and 1.00 atm. What pressure is needed to compress it to 100 cm’ at this temperature? 1.2(a) A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The final pressure and volume of the gas are 5.04 bar and 4.65 dm', respectively. Calculate the original pressure of the gas in (a) bar, (b) atm. 1.3 (a) To what temperature must a 1.0 L sample of a perfect gas be cooled from 25 °C in order to reduce its volume to 100 cm³? 1.4(a) A sample of 255 mg of neon occupies 3.00 dm at 122 K. Use the perfect gas law to calculate the pressure of the gas. 1.7(a) In an attempt to determine an accurate value of the gas constant, R, a student heated a container of volume 20.000 dm³ filled with 0.251 32 g of helium gas to 500°C and measured the pressure as 206.402 cm of water in a manometer at 25°C. Calculate the value of R from these data. (The density of water at 25°C is 0.997 07 g cm; the construction of a manometer is…
The equation of state of a gas is given by . (a) Derive the expression of expansion coefficient in terms of p, V, n, R, T and/or b. (b) Derive the expression of isothermal compressibility a in terms of p, V, n, R, T and/or b. (c) Derive the expression in terms of p, V, n, R, T and/or b. (d) According to the equation of state in this question, is the following statement true or false: based on your results from (a), (b) and (c). Your proof must be based on the results of (a), (b) and (c).
You measure the total pressure of a system is 228.2kPa (P total). You also find there are 49.9kPa (P1) of Hydrogen and 52.9kPa of Carbon (P2). How much Oxygen (P3) is present?
One gram-mole of methyl chloride vapor is contained in a vessel at 100°C and 10 atm.(a) Use the ideal-gas equation of state to estimate the system volume.(b) Suppose the actual volume of the vessel is 2.8 liters. What percentage error results from assuming ideal-gas behavior?
Calculate the molar volume of methane at 300 K and 100 atm given that the second virial coefficient (B’) of methane is -0.0017 atm-1. Assume that all other coefficients are zero. Compare you results with that obtained using the ideal gas equation and the van de Waals Equation of Sate if P =45.4atm;V =0.0990Lmol-1 andT =190.2K
(7) Combustion of CH4 and H₂. For 100 g mol of a gas mixture of 75 mol % CH4 and 25 mol % H₂, calculate the total heat of combustion of the mixture at 298 K and 101.32 kPa, assuming that combustion is complete.