0.58kg argon is compressed polytropic process with n = 1.2 from 125 kPa and 13 ºC in a piston–cylinder device, until its volume is reduced to V2 = c · V1, where the ratio c = 0.5. Ru = 8.314 kJ/(kmol∙K), MAr = 39.948 kg/kmol, cv = 0.3122 kJ/(kg∙K). Argon can be assumed as ideal gas and cv is assumed constant. Determine the final temperature and enthropy change in system

0.58kg argon is compressed polytropic process with n = 1.2 from 125 kPa and 13 ºC in a piston–cylinder device, until its volume is reduced to V2 = c · V1, where the ratio c = 0.5. Ru = 8.314 kJ/(kmol∙K), MAr = 39.948 kg/kmol, cv = 0.3122 kJ/(kg∙K). Argon can be assumed as ideal gas and cv is assumed constant. Determine the final temperature and enthropy change in system

Similar questions

arbon dioxide gas expands from 10.00cm3to 11.50cm3. The final temperature is 450C. Determine the initial temperature if the expansion is elemental.
29) At pressures below about 20 atm, some gas mixtures obey the following equation of state, --—a_p-b_p², where a„ = Σya, and √√5 = ₁√₁. The molar volume of a mixture is i-1 =Ży,f(p.T.y.). V = RT P i-1 given by an expression of the form V = a) Derive the function f(p,T,y).
Problem 2: The specific internal energy and specific volume of liquid water at a temperature of 20.0°C and a pressure of 20.0 MPa are 82.77 kJ/kg and 0.0009928 m³/kg, respectively. Determine the specific enthalpy of the water under these conditions Water u=82.77 kJ/kg v=0.0009928 m³/kg T=20.0°C p=20.0 MPa h=?
140 moles of a gas which has y = 1.31 expands from V₂ = 0.5m³ to Vf = 1.8m³ following the relation P(V) = 2.0 × 105 Pa Pa m³- m³1/1/ +1.2 x 105: m³ 30. What is Cv, the molar specific heat at constant volume, for this gas? (a) 1.3R (b) 2.3R (c) 3.2R (d) 4.2R (e) 5.2R
Two moles of molecular hydrogen (H2) react with 1 mole of molecular oxygen (O2) to produce 2 moles of water (H2O) together with an energy release of 241.8 kJ/mole of water. Suppose a spherical vessel of radius 0.500 m contains 14.4 moles of H2 and 7.2 moles of O2 at 20.0°C. (a) What is the initial pressure in the vessel? (b) What is the initial internal energy of the gas? (c) Suppose a spark ignites the mixture and the gases burn completely into water vapor. How much energy is produced? (d) Find the temperature and pressure of the steam, assuming it’s an ideal gas. (e) Find the mass of steam and then calculate the steam’s density. (f) If a small hole were put in the sphere, what would be the initial exhaust velocity of the exhausted steam if spewed out into a vacuum? (Use Bernoulli’s equation.)
An ideal gas at 20C and a pressure of 1.50x10^5 pa is in a container of volume 6.4dm^3 the number of moles of gas in the container is
If one mole of a monoatomic gas of (y = 5/3) is mixed with one mole of diatomic gas, then the (y = 715) value of y for the mixture will be, (a) 1.5 (b) 1.54 (c) 1.4 (d) 1.45
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
an aluminum aerosol can will burst if the pressure inside reaches 210.0 psi. If the can initially contains an ideal gas at 459.5 kPa at 298.15 K, at what temperature (in K) will the can burst?
2.00-mol of a monatomic ideal gas goes from State A to State D via the path A→B→C→D: State A PA=11.5atm, VA=11.00L State B PB=11.5atm, VB=6.50L State C PC=20.5atm, VC=6.50L State D PD=20.5atm, VD=22.00L Assume that the external pressure is constant during each step and equals the final pressure of the gas for that step. Calculate ΔH for this process.
2.00-mol of a monatomic ideal gas goes from State A to State D via the path A→B→C→D: State A PA=10.5atm, VA=13.50L State B PB=10.5atm, VB=6.00L State C PC=20.5atm, VC=6.00L State D PD=20.5atm, VD=25.00L Assume that the external pressure is constant during each step and equals the final pressure of the gas for that step. A) Calculate q for this process B) Calculate w for this process C) Calculate ΔE for this process D) Calculate ΔH for this process Express answer in L atm units!
(a) Use the ideal gas equation to estimate the temperature at which 1.00 kg of steam (molar mass M = 18.0 g/mol ) at a pressure of 1.50 × 106 Pa occupies a volume of 0.220 m3 . (b) The van der Waals constants for water are a = 0.5537 Pa · m6 /mol2 and b = 3.049 × 10−5 m3 /mol . Use the Van der Waals equation of state to estimate the temperature under the sameconditions. (c) The actual temperature is 779 K. Which estimate is better?