Initially, at a temperature T, and a molar volume vi, a van der Waals gas undergoes...
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between press temperature T for gases better than the Ideal Gas Law does: b) - RT The van der Waals equation of state. R stands for the gas constant and n for moles of gas The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in...
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table...
(a) Show that the entropy change of a Van der Waals gas for an isothermal change V1 to V2 is: ΔS = nR ln (V2 - nb / V1 - nb) (b) Calculate ΔS for expanding on mole of NH3 from 2 dm3 to 20 dm3. Compare this to the ideal gas result. b = 0.0371 dm3/mol
12 This question explores the energy transfer during the reversible isothermal expansion of a van-der-Waals gas. a) The equation of state of the van-der-Waals gas is 141 where Vm is the molar volume. Explain the significance of the constants a and b giving a physical interpretation of both by comparing the equation given with the equation of state of the ideal gas. b) Re-arrange the equation of state given above to produce a formula for the pressure [3] as a...
(30pts) Derive expressions for a gas that obeys the Van der Waals equation of state of (P+a⁄v²)(v-b)=RT where v is specific volume and a and b are constants. For an isothermal process derive expressions to calculate change in enthalpy (h), change in internal energy(u), change in entropy (s),
Two moles of a van der Waals fluid are maintained at a temperature T = 0.95TC in a volume of 200cm3. At this temperature, the reduced molar volume of the liquid phase νl ~ 0.68 and that of the gas phase νg ~ 1.7. Assuming the substance to be oxygen (i.e., using the van der Waals constants for oxygen a = 0.138 Pa-m6 and b = 32.6x10-6m3), find the mole number and volume of each phase.
A van der Waals gas undergoes an isothermal reversible compression under conditions such that z=0.95. What is the ratio of the work for this process compared to the work for the same process with an ideal gas?
Use the van der Waals equation and the ideal gas equation to calculate the volume of 1.000 mol of neon at a pressure of 500.0 bar and a temperature of 355.0 K. (Hint: One way to solve the van der Waals equation for V is to use successive approximations. Use the ideal gas law to get a preliminary estimate for V ITS 500BAR use bar please not ATM
A van der Waals gas has an "a" constant of 1.485 L' atm mol2 and a"b' constant of 3.985 x 102 L mori, calculate the value of-( )(or), for this van der Waals gas at a molar volume of 450 cm3 mol1 and a temperature of 100 °C. Include units
4. A certain gas obeys the van der Waals equation with a = 0.76 m Pa mol-?. Its volume is found to be 3.50 x 10 m mol-1 at 236 K and 4.1 MPa. 1) From this information calculate the van der Waals constant b. 2) What is the compression factor for this gas at the prevailing temperature and pressure?