An ideal gas described by
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Thermodynamics, Statistical Thermodynamics, & Kinetics
- 5. An ideal gas described by Ti= 275 K, Pi = 1.10 bar, and Vi = 10.0 L is heated at constant volume until P = 10.0 bar. It then undergoes reversible isothermal expansion until P = 1.10 bar. It is then restored to its original state by the extraction of heat at constant pressure. Depict this closed-cycle process in a P-V diagram. Calculate w for each step and for the total process.arrow_forward= 1.10 bar, P2.19 An ideal gas described by T; = 275 K, Pi and Vi = 10.0 L is heated at constant volume until P = 10.0 bar. It then undergoes a reversible isothermal expansion until P = 1.10 bar. It is then restored to its original state by the extraction of heat at constant pressure. Depict this closed-cycle process in a P-V diagram. Calculate w for each step and for the total process. What values for w would you calculate if the cycle were traversed in the opposite direction?arrow_forwardAt 25 °C, the equilibrium partial pressures for the reaction A(g) + 2 B(g) 4 C(g)+D(g) were found to be PA = 4.45 bar, Pg = 5.82 bar, Pc = 5.74 bar, and Pp = 4.05 bar. %3D %3D What is the standard change in Gibbs free energy of this reaction at 25 °C?arrow_forward
- 6A. State whether each of the following is true or false. Explain your reasoning in each case. (a) q must be zero for an isothermal process (b) q=0 for every cyclic process [A cyclic process is one that begins in one state and undergoes several steps which ultimately bring the system back to the same initial state.] (c) DU=0 for every cyclic process. (d) DT=0 for every adiabatic process in a closed system.arrow_forwardElement X has an enthalpy of fusion of 59.2 kJ mol-1 at its melting point (684°C). Calculate ΔSsys for the process,X(l) → X(s)At 1 bar and 684°C. Express your answer in units of J mol-1 K-1 to 3 significant figures.arrow_forwardCalculate the change in enthalpy when 124 g of liquid methanol initially at 1.00 bar and 298 K undergoes a change of state to 2.50 bar and 425 K. The density of liquid methanol under these conditions is 0.791 g cm-3, and Gp, m for liquid methanol is 81.1 JK1 mol1. Molar mass (methanol) = 32.04 g mol 1arrow_forward
- Carbon dioxide gas with a mass of 88 g is isothermally compressed at a fixed external pressure of 15 bar, with a speed of 298 K and a final pressure of 10 bar from 1 bar. Interpret the results by finding the quantities Δu, Δh, w, Q, Δs, Δa, g and Δsaverage, Δssystem in the event.arrow_forwardThe constant-pressure heat capacity of a sample of a perfect gaswas found to vary with temperature according to the expression Cp/(J K−1) = 20.17 + 0.3665(T/K). Calculate q, w, ΔU, and ΔH when the temperature is raised from 25 °C to 100 °C (i) at constant pressure, (ii) at constant volume.arrow_forwardThe atomic heat capacity of solid Mo is given by the equation 0.503 x 105 Cp = 5.69 + 1.88 x 10-3 T – T² Find the change in entropy (in eu) which accompanies the heating of one mole of Mo from o C to its melting point, 2620°C. (Entropy unit, (eu) equal to i cal K-¹). Cp expression gives heat capacity in units of cal/mol.arrow_forward
- Calculate ΔS (for the system) when the state of 2.00 mol of gas molecules, for which Cp,m = R, is changed from 25 °C and 1.50 atm to 135 °C and 7.00 atm.arrow_forward1.4 g of N2 are placed in a cylinder at an initial volume of 3.8 L and allowed to expand isothermally to a final volume of 10.8 liters against a constant external pressure of 0.8 bar. (A) Treating N2 as a perfect gas, find q, w, ΔU, ΔH, and ΔS for this process. (B) Now assume that the same process occurs, but that N2 can be assumed to have attractive forces between the molecules. In this case, how would q differ from the answer given in (A)? Specifically, would the value be larger, smaller, or unchanged? Explain your answer in 10 words or less. Can you please explain part a and b? <reference> Ne has a mass of 20.18 amu, N2 has a mass of 28.01 amu, H2 has a mass of 1.01 amu, Ar has a mass of 39.95 amu, and He has a mass of 4.00 amu.arrow_forwardCalculate the change in entropy of the system when 10.0 g of ice at −10.0 °C is converted into water vapour at 115.0 °C and at a constant pressure of 1 bar. The molar constant-pressure heat capacities are: Cp,m(H2O(s)) = 37.6 J K−1 mol−1; Cp,m(H2O(l)) = 75.3 J K−1 mol−1; and Cp,m(H2O(g)) = 33.6 J K−1 mol−1. The standard enthalpy of vaporization of H2O(l) is 40.7 kJ mol−1, and the standard enthalpy of fusion of H2O(l) is 6.01 kJ mol−1, both at the relevant transition temperatures.arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,