A 2.25 mole sample of an ideal gas with
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Thermodynamics, Statistical Thermodynamics, & Kinetics
- 3. What is the change in entropy associated with heating water from 15 ºC to 55 ºC? The constant volume heat capacity of water is CV,m = 75.3 J/mol K, and is constant over this temperature range.arrow_forwardWhat is the reversible work, in joules, for the expansion of 2.50 mol of an ideal gas from 4.7 bar to 1.65 bar at a constant temperature of 298 K.arrow_forwardThe molar heat capacity of oxygen at constant pressure can be expressed as follows: Cp,m = a + bT, where a = 6.15 cal mol-1 K-1and b = 0.0031 cal mol-1 K-2. a) 2 mols of oxygen have been heated up reversibly from 27 ºC to 127 ºC, at a constant pressure of 1 atm. Calculate the w, q, ΔU and ΔH of the process. b) Same thing, assuming an isocoric process. The oxygen behaves as an ideal gas.arrow_forward
- A monatomic perfect gas at a temperature T; is expanded isothermally to twice its initial volume. To what temperature should it be cooled to restore its entropy to its initial value? Take Cv,m = (3)/(2)R.arrow_forwardThe standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are -238.7 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol respectively. Calculate the change in surrounding entropy (in J/K) during combustion of 12.7 g of methanol under a constant pressure of 1,000 atm at 25.00 oC (N.B., combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).arrow_forwardEstimate the standard internal energy of formation of liquid methyl ethanoate, CH3COOCH3, at 298 K from its standard enthalpy of formation, which is -442 kJ mol-1.arrow_forward
- In the isothermal reversible compression of 52.0 mmol of perfect-gas molecules at 260 K, the volume of the gas is reduced from 300 cm3 to 100 cm3. Calculate the magnitude of the work done for this process.arrow_forwardIf 2 mol of neon (assumed ideal) is heated from 0 °C to 250 °C at a constant pressure of 1 bar, calculate the values of q, w, ∆U, and ∆H. (b) calculate the values of q, w, ∆U, and ∆H for the same neon sample heated to 250 °C at a constant volume from the same initial condition and then isothermally expanded to the same final volume as in part 1. (a). For the melting of 100 g of ice at 0 °C and a constant pressure of 1 bar, calculate q, w, AU, and AH. Ice has a density of 0.916 g/mL1. (a) Calculate the value for q, w, AU, and AH vaporizing 2 mol of liquid water is converted to steam at 100 °C under a constant pressure of 1 bar. From a temperature of 453.15 K and a volume of 15 dm3 (state 1), a sample of 2 mol of argon gas is expanded adiabatically and reversibly to a final temperature of 400 K. (state 2). Calculate the process's final volumes V2, ∆U, ∆H, w, and q.(b) Consider an irreversible adiabatic expansion with the same initial state and the same final volume, carried out with…arrow_forwardAn electrical heater delivers 6.800 kJ of energy (as heat) to a system consisting of the gas inside a cylinder having a movable piston. As a result, the piston moves against a constant external pressure such that P ∆V = 2.720 kJ. What is the change in internal energy for the system? Answer to the nearest 0.001 kJ.arrow_forward
- A sample of a serum of mass 26.6 g is cooled from 290 K to 275 K at constant pressure by the extraction of 1.05 kJ of energy as heat. Calculate q and ΔH and estimate the heat capacity of the sample. report here the heat capacity = ________ J/k/g. 3 sig. numberarrow_forwardThe standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are, respectively, -238.7 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the change in the entropy of the surroundings (in J/K) upon the combustion of 13.3 g of methanol under a constant pressure of 1.000 atm and a temperature of 25.00 oC. N.B. combustion is the reaction of this substance with molecular oxygen to produce water and carbon dioxide.arrow_forwardWhen 2.0 mol of CO2 is heated at a constant pressure of 1.25 atm, its temperature increases from 280.00 K to 307.00 K. The heat (q) absorbed during this process is determined to be 2.0 kJ. Calculate (a) ΔH for this process (b) The molar heat capacity of CO2 at constant pressure (CP,m) (Hint: you can assume that CP,m is constant over this temperature range and that the CO2 behaves ideally). (c) ΔU.arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning