4.11. Consider a piston whose compression ratio is 10:1; that is, Vf = 10 X V₁. If 0.0200 mole of gas at 1400 K expands reversibly, what is AA for one expansion of the piston?
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Confused with pchem. I don't know how to find v initial
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- 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 solutionsA sample consisting of 1.00 mol Ar is expanded isothermally at 20 degrees celsius from 10 dm^3 to 30dm^3 (a) reversibly, (b) against a constant external pressure equal to the final pressure of the gas, and (c) freely aka - against zero external pressure. For the three processes calculate q,w, and delta UThe heat capacity ratio of an ideal gas is 1.38. What are its Cv and Cp values?
- 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 sample consisting of 2.00 mol of perfect gas molecules, for which CV,m = 5/2R, initially at p1 = 111 kPa and T1 = 277 K, is heated reversibly to 356 K at constant volume. Calculate the final pressure, ΔU, q, and w.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?
- Everything needed is included Consider the reversible and isothermal compression of 2.0 moles of ammonia (NH3 (g)) from an initial volume of 10.0 L to a final volume of 1.00 L, at a constant temperature of 298 K: 6a. Calculate the work w and heat q associated with this change in volume, considering NH3 to be an ideal gas. 6b. Calculate the work w (but not the heat) using the virial equation of state, with second virial coefficient B = −0.297 L/mol for NH3 at this temperature (and ignoring any higher coefficients).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 adiabatic: 1) ΔT 2) q 3) w 4) ΔU 5) ΔH1.65 mol of a perfect gas for which Cv,m = 12.47 J K–1 mol–1 is subjected to two successive changes in state: (1) from 37.0 oC and 1.00´105 Pa, the gas is expended isothermally against a constant pressure of 16.5´103 Pa to twice its initial volume. (2) At the end of the previous process, the gas is cooled at constant volume from 37.0 oC to - 23.0 oC. (a) Calculate q , w , DU, DH for each of the stages.