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A 2.25 mole sample of an ideal gas with
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Chapter 2 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
- Benzoic 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_forwardThe 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_forwardWhat is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?arrow_forward
- Calculate the change in molar enthalpy DHm when the given gas is heated from 25 oC to 500 oC using the expression above. The constants a, b, and c are available in Table 2B.1.arrow_forwarda) 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_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
- What 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_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_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_forward
- A 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_forwardKnowing 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_forwardConsider the expression: dS=dT - VadP. Suppose that water has ß = 4.53x10-5 atm¯¹, V = 18 cm³/mol, C = 18 cal/deg-mol, and a = 2.0 x10 deg¹. Compute the decrease in temperature which occurs if water at 25 °C and 1000 atm pressure is brought reversibly and adiabatically to 1 atm pressure.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
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