A 2.25 mole sample of an ideal gas with
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Thermodynamics, Statistical Thermodynamics, & Kinetics
- The Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants determined experimentally. For NH3g, a = 10.91 atm. L2 and b = 0.0401 L. Plot the pressure of the gas as the volume of 1.00 mol of NH3g expands from 22.4 L to 50.0 L at 273 K, and numerically determine the work done by the gas by measuring the area under the curve.arrow_forwardBenzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.arrow_forwardWhat is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?arrow_forward
- F-2 8. A 3.50 mole sample of an ideal gas with Cv= 3R/2 undergoes reversible expansion. The initial temperature and pressure are T1 = 310 K and P1 = 15.2 bar. The final pressure is P2 = 1.45 bar. Calculate ΔU in kJ for this process. (First calculate T2) Please show all steps.arrow_forwardTwo moles of an ideal gas are expanded reversibly and isothermally at 0 °C from 1 atm. Calculate the final volume (in L) occupied by the gas if the heat absorbed during the process is 750 cal.arrow_forward6E. A 2.25 mole sample of CO,(g), for which C,.m=37.1 J/K at 298 K, expands reversibly and adiabatically from a volume of 4.50 L and a temperature of 298 K to a final volume of 32.5 L. Calculate the final temperature, q, w, AH and AU for the process. Assume that the gas behaves ideally and that C. is p.m constant over this temperature interval.arrow_forward
- a) Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2. Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units. (b) Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K. (c) Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.arrow_forwardWhat if we assumed that the heat capacity of gaseous NH3 is NOT dependent on temperature? Calculate the energy per mole required to be removed from gaseous NH3 from decrease the temperature of the system from 400 °C to 25 ºC. Assume that the heat capacity, Cpm, of NH3 is a constant over the temperature range considered and can be found in Table 2C.7arrow_forwardFive moles of monatomic ideal gas enter the abc cycle and during a complete cycle 600 J of heat is removed from the gas. Process ab is under constant pressure and process bc is increasing at constant volume takes place at pressure. The temperatures of points a and b are Ta= 3°C and Tb= 63°C. What is the work in the ca process?arrow_forward
- Knowing that the molar heat capacity at constant pressure of CO₂ has the form Cp,m = (a + b + c/T²) J mol-¹K-¹, where a= 44.22, b= 8.79 x 10-³ K-¹, and c= -8.62 x 105 K 2,calculate how much heat can absorb 1.5 moles of this gas when the temperature is increased from 25°C to 150°C. NOTE: Give your answer in kJ mol-1arrow_forwardA sample of 3.0 moles of an ideal gas at 200 K and 200.0 kPa is compressed reversibly and adiabatically until the temperature reaches 250 K. Given the molar heat capacity at constant volume is 27.5 J K-1 mol-1, calculate q, w, delta U, delta H, the final pressure and the final volume. the correct answers are 0 J; 1.87 kJ; 1.87 kJ; 3.1112 kJ but I am getting a different answers insteadarrow_forwardSuppose 2.00 mol of a monatomic ideal gas (cy = }R) is expanded adiabatically and reversibly from a temperature T = 300 K, where the volume of the system is 20.0 L, to a volume of 60.0 L. Calculate the final temperature of the gas, the work done on the gas, and the energy and enthalpy changes.arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning