For which of the following processes is the equation AS = qrev /T valid? 4. any reversible expansion of an ideal gas. isothermal irreversible compression of a non-ideal gas. constant pressure heating of a liquid. isothermal vaporization of a liquid. isothermal sublimation of a solid to a non-ideal vapor. 1. 2. 3. 4. 5. 1 & 3 only B) 1, 4 & 5 only E) 4 & 5 only C) 2, 3 & 4 only A) D) 2, 4 & 5 only
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- 3 m of an ideal gas expands from 400K and 4 bar to 1 bar final pressure. --- The situation where the expansion is isothermal and reversible --- The situation where the expansion is adiabatic and reversible Explain which job is bigger and why by finding job values for situations. Cv, m = 3 / 2RA sample containing 2.05 moles of an ideal gas with CV = 20.1 J K-1 is initially at 3.84 bar and 300. K. It is compressed at constant volume until its pressure reaches 5.62 bar. Calculate the final temperature, work done, heat transferred, ΔU, ΔH and ΔS for the process.Which of the following statements is/are true? You may select more than one, or none, of the options. ΔSuniv = 0 for an adiabatic process. ΔSsurr = 0 for a reversible process. ΔSsurr = 0 for an adiabatic process. ΔS = 0 for an adiabatic process. ΔSuniv = 0 for a reversible process. ΔS = 0 for a reversible process.
- A piston/cylinder setup contains 1 kg of air at 20°C with an initial volume of V1=0.1 m3, as shown in Fig. Q7. Initially, the piston rests on some stops, but it is possible for it to move within the cylinder without friction. To lift the piston and start such motion, an air pressure of 1400 kPa is required. Now, heat is transferred to the system so that the temperature of the air reaches to a final value of 300°C. Fig. Q7 A. Which statement is true? The air can lift the piston before the temperature reaches to 300°C The air cannot lift the piston before the temperature reaches to 300°COne mole of nitrogen (N2) is cooled from an initial temperature and pressure of 700 K and 10 bar to a final temperature of 300 K. The heat capacity of nitrogen may be taken as: Cp,m = 28.58 + 3.77 × 10-3 T where Cp,m is in J mol-1 K-1 and T is in Kelvin. Assuming nitrogen behaves as an ideal gas, calculate q, w, ∆U, and ∆H for this process when it is carried out (a) at constant pressure, and (b) at constant volume. Compare the values obtained for the two cases.1 kg of Air was heated at constant temperature from 0.03 m3 and 101 kPa to 0.01 m3. By how much did the internal energy change? Assume (cv = 0.7177 kJ/kg.K)
- The n-butane is converted into isobutane in an isomerization reactor, which operates isothermally at 149°C. Suppose that the reactor is fed with a mixture containing 93% mole of n-butane, 5% isobutane and 2% HCl at 149°C and that a 40% conversion of n-butane is achieved. How much heat in KJ/m3 (STP) of the feed, should be supplied or extracted from the reactor?How would an ideal gas (where dU=Cv(dt) is always true) undergoing isothermal reversible expansion be represented by the equation for the First Law? Think about what is changing in order to do work. Which term(s) is/are now zero?1.50 mol of an ideal gas undergo a reversible isothermal expansion from 1.80 dm3 to 2.80 dm3. What is S, Ssurr, and Stot ? (b)If the expansion in (a) is free, What is S, Ssurr, and Stot ? Q2. (5 marks) Calculate S when 0.0385 mol of an ideal gas (Cv,m = 1.5R) at 20.0oC and 1.30 atm expand to 0.900 atm and, at the same time, cool to ‒21.5 oC.
- One mole (1.0 mol) of an ideal gas is initially at T1 = 298 K and has volume V1 = 2.0 L. It is then reversibly expanded to final volume V2 = 3.0 L. Assume Cp = 5/2 R and Cv = 3/2R. a) Calculate the following if the expansion is isothermal: 1) ΔT 2) q 3) w 4) ΔU 5) ΔH b) Calculate ΔT–ΔU if the expansion is adiabatic instead of isothermal.c) Calculate the initial pressure and two final pressures for the process in a) & b).d) On a single set of axes, sketch a pressure–volume plot for each of the two processes in a) & b). Label the area that corresponds to the work for each process.Calculate Q (system) (J) and delta H (kJ/mol). Use data below and from methods: Mass of NaNO3 required (already calculated) = 8.5 grams Initial Temperature ti (0C) = 25.0 0C Temperature after 240 sectons (tf, final temp) = 19.0 0C Measuring the heat evolved or absorbed methods Weigh the calculated mass of NaNO3 needed to prepare 100mL of a 1.0M solution. Place 100mL of distilled water in the calorimeter and carefully add the solid NaNO3. Begin stirring and measure the temperature of the solution to the nearest 0.10C after 30seconds and every 30 seconds thereafter until the temperature attains either a maximum or minimum which is the final temperature tf. Calculate q(system), using specific heat=4.184J/g.0C, density ofsolution=1.0g/mL; heat capacity of calorimeter = 10J/0C Calculate the enthalpy change DH from q(system) and the number of moles NaNO3Find change in Ssys,change in Ssurr, q, w, and change in U for the reversible isothermal expansion of 3.000 mol of argon (assumed ideal) from a volume of 100.0 L to a volume of 500.0 L at 298.15 K.