(b) An ideal gas of 2.5 moles undergoes an adiabatic expansion at an initial pressure of 4.25 bar and at an initial temperature of 540 K to a final temperature of 400 K. Calculate the work done which is equal to internal energy change under such conditions. Assume Cp,m = 5/2 R %3D
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- What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units of cal/mol.K and L.atm/mol.K?A sample of nitrogen of mass 3.12 g at 23.0 °C is allowed to expand reversibly and adiabatically from 400 cm3 to 2.00 dm3. What is the work done by the gas?Calculate the molar heat capacity at constant pressure (Cp) for a diatomic H2 gas(y = 1.41) with molar heat capacity at constant volume (Cv) of 20.42 J/mol-K?
- What would be the final volume occupied by 1.0 mol of an ideal gas initially at 0°C and 1.0 bar if Q = 1000J during a reversible isothermal expansion?A 1.5 mol of perfect gas molecules with Cpm = 20.8) K-1 mol-1 is initially at 230 kPa and 315 K. It undergoes reversible adiabatic expansion until its pressure reaches 170 kPa. Calculate the final volume and temperature and the work doneCalculate the work done during the isothermal reversible expansion of a gas that satisfies the virial equation of state (eqn 1C.3b) written with the first three terms. Evaluate (a) the work for 1.0 mol Ar at 273 K (for data, see Table 1C.3) and (b) the same amount of a perfect gas. Let the expansion be from 500 cm3 to 1000 cm3 in each case.
- The equation of state for a certain gas is given by P[(V/n)-b] = RT. Obtain an expression for the maximum work done by the gas in a reversible isothermal expansion from V1 to V2.(b) An ideal gas of 2.5 moles undergoes an adiabatic expansion at an initial pressure of 4.25 bar and at an initial temperature of 540 K to a final temperature of 400 K. Calculate the work done which is equal to internal energy change under such conditions. Assume Cp,m = 5/2 RA mole of an ideal, diatomic gas undergoes isothermal, reversible expansion from 1.0 dm^3 to 10.0 dm^3 at 100°C. if the same gas undergoas irreversible expansion against a constant pressure of 1.00 bar, which of the following quantities would change? A. Internal energy B. Entropy C. Free energy D. Enthalpy
- A perfect gas (Cv= 3R/2) is expanded in a reversible adiabatic processfrom a volume of 2 L, at 2 atm and 300 K, until a final temperature which isthe four times smaller than the initial one. Calculatea) The final volume and pressureb) the work and the internal energy variation of the transformationA sample of 2.2 mol CO2(g) is originally confined in 15 dm3 at 280 K and then undergoes adiabatic expansion against a constant pressure of 78.5 kPa until the volume has increased by a factor of 4.0. Calculate ΔT. (The final pressure of the gas is not necessarily 78.5 kPa.)One mole of a perfect monatomic gas, initially at 300 K and a pressure 15.0 atm, expands to afinal pressure of 1.00 atm. Consider the expansion via each of the following paths: (a)isothermal and reversible, (b) isothermal and irreversible, (c) adiabatic and reversible, (d)adiabatic and irreversible. In these irreversible processes, the expansion occurs against anexternal pressure of 1.00 atm. For each case, calculate the values of q, w, ΔU and ΔH.