Initially at 300 K and 10 atm pressure, 1 mol ofa gas is allowed to expand adiabaticallyagainst a constant pressure of 4 atm untilequilibrium is reached.Assume the gas to be ideal withCp,m (J K-1) = 28.58 + 1.76 x 102 T (K)and calculateAU, AH, AS

It is important to know that a process without transfer of heat to or from a system, so that Q = 0,…

Answered: Initially at 300 K and 10 atm pressure,…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 32QAP

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Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
(1) Calculate AG for the following reactions at the stated temperatures: (a) ZnO(s) + C(s) Zn(s) + CO(g) at 298 K, when AH08 +238.6 kJ mol; AS = +213 J K mol. (b) ZnO(s) + C(s) Zn(g) + CO(g) at 1373 K, when An = +349.9 kJ mol; AS3 = +285 J K- mol. (c) Fe(s) + 0,(8) FeO(s) at 298 K, when AH298 = -265.4 kJ mol; ASOR = -71 J K mol.
The reduction of iron(III) oxide (Fe,0,) to pure iron during the first step of steelmaking, 2 Fe,0, (s) – - 4 Fe(s) + 30,() is driven by the high-temperature combustion of coke, a purified form of coal: 圖 C(s) + 0,(g) → Co, (g) dlo Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO, and Fe, O, are -428. kJ/mol and -833. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 2000. kg of pure iron. Round your answer to 2 significant digits. Okg Explanation Check O 2021 McGraw-Hill Education. AlI Rights Reserved. Terms of Use| Privacy | Accessibility
3. One mole of liquid water at 100 °C is heated until the liquid is converted entirely to vapor at 100 °C and 1 atm pressure. Calculate q, w, AE and AH for each of the following. (a) The vaporization is carried out in a cylinder where the external pressure on the piston is maintained at 1 atm throughout. (b) The cylinder is first expanded against vacuum (Pext = 0) to the same volume as in part (a), and then sufficient heat is added to vaporize the liquid completely to 1 atm pressure.
The following gaseous system is in equilibrium at 30.00C and 1 bar, where 25% of N2O4 is dissociated into NO2: N2O4(g) 2 NO2(g) (a) Calculate the equilibrium constant, K. (b) Calculate the extent of the dissociation, a at 30.00C and 0.1 bar.
In a particular biokgikal reaction taking place in the body at 37 C, the change in enthalpy was -125 kJ mol' and the change in entropy was -126 JK' mol". (a) Cakulate the change in Gibbs energy. (b) Is the reaction spontaneous? (e) Cakulate the total change in entropy of the system and the surroundings.
From the following data determined at 298 K, determine (a) A, H and A₁U for reaction (4) at 298 K; (b) AfH for HI(g) and H₂O(g) at 298 K. Assume ideal gas behavior when necessary. (1) H₂(g) + I2(g) → 2 HI(g) (2) 2H₂(g) + O₂(g) → 2H₂O (g) (3) 1₂ (s)→ I2(g) (4) 4HI(g) + O₂(g) → 21₂(g) + 2H₂O(g) ΔΗΘ = +52.96 kJ mol-¹ A₂H = -483.64 kJ mol-1 A₂H = +62.44 kJ mol-¹
In a particular biological reaction taking place in the body at 37 °c, the change in enthalpy was -135 kJ mol-1 and the change in entropy was - 136 J K-1 mol-1. (a) Calculate the change in Gibbs energy. (b) Is the reaction spontaneous? (c) Calculate the total change in entropy of the system and thesurroundings.
Indicate whether each statement is true or false. (a) Thethird law of thermodynamics says that the entropy of aperfect, pure crystal at absolute zero increases with themass of the crystal. (b) “Translational motion” of moleculesrefers to their change in spatial location as a functionof time. (c) “Rotational” and “vibrational” motionscontribute to the entropy in atomic gases like He and Xe.(d) The larger the number of atoms in a molecule, themore degrees of freedom of rotational and vibrationalmotion it likely has.
(a) Under what conditions is a dA < 0 condition thatdefines the spontaneity of a process?(b) A sample containing 2.50 moles of He (1 bar, 350. K) ismixed with 1.75 mol of Ne (1 bar, 350. K) and 1.50 mol ofAr (1 bar, 350. K). Calculate AGmixing and ASmixing.
(d) For the reaction: H3C. H3C. C-OH Cc=CH2 H3C H20 H,C H3C Reaction 2 Reaction 2 does not go to completion and the position of the reaction can be defined in terms of the equilibrium constant, K. (i) For the above reaction at 298K under specific conditions the following thermodynamic information were obtained, reaction Gibbs free energy (AreactG = -5.4 kJ mol-1), standard reaction enthalpy (AreactH® = -52.7 kJ mol-1) and standard reaction entropy (AreactS® = -0.16 kJ mol-1). From the above detail, calculate the equilibrium constant. (ii) Sketch a diagram of the Gibbs free energy versus reaction progress and on diagram label the reaction Gibbs free energy (A,react G) and standard reaction Gibbs free energy (Areact G®).
6. When the ideal-gas reaction A+B=C+Dhas reached equilibrium, state whether or not each of the following relations must be true. Here n¡ is the number of moles of species i in equilibrium, P, is the partial pressure of i, and µ; is the chemical potential of i. Here a simple True or False answer is sufficient. (a) nc+np=nA +ng (b) Pc+Pp=PA+PB (c) na=ng (d) nc=na (e) If only A and B are present initially, then nc=np (f) Ha + HB= Hc+ Hp no matter what the initial composition. (g) If only A and B are present initially, then in equilibrium we must have nc # 0. (h) The equilibrium constant Kp(T)= PĄPB/(PcPp). (i) The value of –RT In Kp(T) = µE(T)+µ8(T)– H3(T) –- H§(T). ) The equilibrium constant is independent of the total pressure.

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Initially at 300 K and 10 atm pressure, 1 mol of a gas is allowed to expand adiabatically against a constant pressure of 4 atm until equilibrium is reached. Assume the gas to be ideal with Cp,m (J K-1) = 28.58 + 1.76 x 102 T (K) and calculate AU, AH, AS