When burned Propane in air, the approximation mole fraction analysis of production gases is xCO₂=0.1055, xH₂O=0.14, xO₂=0.0195, xN₂=0.7344. Fined the adiabatic flame temperature?
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- P2.30 A 1.75 mol sample of an ideal gas for which Cv.m = 3R/2 undergoes the following two-step process: (1) From an initial state of the gas described by T = 15.0°C and P = 5.00 X 104 Pa, the gas undergoes an isothermal ex- pansion against a constant external pressure of 2.50 × 104 Pa until the volume has doubled. (2) Subsequently, the gas is cooled at constant volume. The temperature falls to -19.0°C. Calculate q, w, AU, and AH for each step and for the overall process.The temperature change associated with the adiabatic expansion of an ideal gas is defined as: Trinal = Tinitial (Vinitial / Vfinal)V where: Tinitial and Tfinal are the temperatures before and after the adiabatic expansion respectively; Vinitial and Vfinal are the volumes before and after the adiabatic expansion respectively; c = Cm/R; where Cmvis the molar isochoric heat capacity and R is the universal gas constant. Which of the following is true? O A. The higher the amount of the ideal gas, the greater the temperature change. O B. The higher the amount of the ideal gas, the smaller the temperature change. O C. The final volume is lower than the initial volume. O D. The temperature change is independent of the amount of the gas involved. E. The temperature change is inversely proportional to the molar isochoric heat capacity of the gas.A pellet of naphthalene (C10H8, MW = 128.19) of mass 1.234 g is burned in a bomb calorimeter with Ccal = 14225 J K-¹. If the initial temperature is 296.15 K and the final temperature is 301.634 K, find AH (in kJ) for 1 mol of reaction, with liquid water as one of the products. Neglect the heat of combustion of the wire fuse.
- 1. A real gas obeys the following equation of state, where ß is a positive constant. BP PV = nRT T (a) Show that (3P) = μCp T (b) Find the expression for Joule Thomson coefficient for this gas in terms of constant B and heat Cp of the gas. (c) Does the temperature of the gas increase or decrease? Give reason.(a) 2 mole of an ideal monoatomic gas at 27°C expands reversibly and adiabatically from a volume of 20 dm to a volume of 40 dm2. Calculate q. AU, W and AH. Given CR= 4/3Benzoic acid, C;HsO:H, is typically used as a çalibrant for determining the specific heat of bomb calorimeters. It combusts via the following unbalanced chemical reaction: C,H5O2H (s) + 02(g) → CO2 (g) + H2O(1) 3. For this experimental setup and reaction, the constant volume heat flow is known to be gy = -26.979 kJ. Over the course of the reaction, the temperature rose from 19.863 °C to 22.540 °C. Calculate the heat capacity, Cou, for this calorimeter in kJ °C-!.
- Two moles of an ideal gas with cP=72R= 29.10 J mol-1 K-1 are at initial pressure p1= 1 atm and temperature T1 = 295 K. The gas undergoes two different processes from this particular initial state (1) Heating under constant volume to a final temperature of 405 K. Calculate the quantities AU, AH, AS, q and w (2) Adiabatic and irreversible change at a final temperature of 100 K. Calculate the quantities AU, AH, AS, q and w (1) (2) AU ΔΗ AS 9 WP3A.2 A sample consisting of 0.10 mol of perfect gas molecules is held by a piston inside a cylinder such that the volume is 1.25 dm²; the external is constant at 1.00 bar and the temperature is maintained at 300 Kby a thermostat. The piston is released so that the gas can expand. Calculate (a) the volume of the gas when the expansion is complete; (b) the work done when the gas expands; (c) the heat absorbed by the system. Hence calculate ASor pressureTwo ideal gases, one monoatomic and the other diatomic are mixed with one another and form an ideal gas again. The equation of the adiabatic process of the mixture is 11 PVY= = constant; where What is the ratio of the number of molecules of the monoatomic gas to that of the diatomic gas in the mixture?
- The molar heat capacity CPm of H2(g) is described by the following equation.: CPm = 29.064 -0.8363x10-3 TIK + 20.111x10-7 (TIK)? In this equation, T is the absolute temperature in kelvin. The ratios (TIKY" ensure that Cpm has the correct dimension. Assuming ideal gas behavior, calculate q, w, AU, and AH if 2.5 moles of H2(g) is heated from 25 °C to 800 °C at a constant pressure of 1 bar. q (in J) = w (in J) = AU (in J) = AH (in J) =You have four samples of ideal gas, each of which contains the same number of moles of gas and has the same initial temperature, volume, and pressure. You compress each sample to one-half of its initial volume. Rank the four samples in order from highest to lowest value of the final pressure. (i) A monatomic gas compressed isothermally; (ii) a monatomic gas compressed adiabatically; (iii) a diatomic gas compressed isothermally; (iv) a diatomic gas compressed adiabatically.The constant pressure molar heat capacity of nitrogen is given by the expression: Cp,m = 27.0 + 5.90 x 10-3 T - 0.34 × 10-6 T²JK1 mol1 Calculate the value of AH for heating 1 mole of nitrogen from 17.7° C to 138.5°C. Express your answer in Joules to the first decimal place (XXXX.X).