Given the following reaction at 298 K:2 H2S(g) + SO2(9) → Ss(s) + 2 H20(g)Part AArG" = -102 kJ molDetermine the value of the reaction quotient Q when: Pu,s = 2.00 bar; Pso, = 0.185 bar; and Pa,0 = 1.245 baExpress your answer using three significant figures.fe kevboard shortcuts helpTemgrates Symbols undo regoQ =

Consider the given reaction at 298 K is as follows; 2 H2S g + SO2 g → 38 S8 s + 2 H2O g…

Given the following reaction at 208 K: 2 H2S(9) + SO2(g) → Sa(s) + 2 H2O(g) Part A AG" =-102 kJ mol Determine the value of the reaction quotient Q when: Ps = 2.00 bar: Pso, = 0.185 bar; and Pi,o = 1.245 bar Express your answer using three significant figures.

Given the following reaction at 208 K: 2 H2S(9) + SO2(g) → Sa(s) + 2 H2O(g) Part A AG" =-102 kJ mol Determine the value of the reaction quotient Q when: Ps = 2.00 bar: Pso, = 0.185 bar; and Pi,o = 1.245 bar Express your answer using three significant figures.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For the reaction P4010(s) + 6 H20(1) 4 H3PO4(aq) AG° = -448.9 kJ and AS° = -16.3 J/K at 261 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 261 K. The standard enthalpy change for the reaction of 2.15 moles of P4010(s) at this temperature would be kJ. Submit Answer Try Another Version 1 item attempt remaining rch a
Consider the following reaction: CO2 (g) + CCI4 (9) = 2COCI, (g). Part A Calculate ArG for this reaction at 125 °C under the following Poo, = 0.135 bar POCI, = 0.160 bar PoOCI, = 0.755 bar conditions. ? A;G = - 10.830 kJ mol-1 Submit Previous Answers Request Answer X Incorrect; Try Again
Calculating dG from dH and dS A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 59.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. alo AH = -172. kJ J AS = -420. K CH, OH (g) + CO(3) - HCH,CO, (1) AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither AH =…
Gaseous SO2Cl2 reacts with liquid water to form hydrogen chloride gas and liquid sulfuric acid. Using data tabulated in Appendix G of your text, calculate the enthalpy change, in units of kJ/mol, for the formation of 2 mol of liquid sulfuric acid.
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 achieved. Assume the gas to be ideal with Cp,m = 28.58 + 1.76 x 10^-2 T(The units of T are K and the units of Cp,m are J K-1 mol-1.) Compute DU, DH, q and w.
The equilibrium reaction for the aqueous dissociation of acetic acid is shown below. CH3COOH(aq) = CH3COO-(aq) + H+ (aq) Given the data in the table below and your knowledge of the "chemical standard state" (X) and the "biochemical standard state” (Xº'), answer parts a) to e). Gibbs free energy of formation, in units of kJ mol-1, at T = 298.15 K AfGe A¢G° -396.5 -369.3 0 CH3COOH(aq) CH3COO- (aq) H+ (aq) d) For the dissociation of acetic acid at 298.15 K, calculate A,Gº¹. 0
From these two reactions at 298 K,
Calculate ASor for the reaction 3H2(g) +N2(g) → 2NH3(g) at 744 K. Omit terms in the temperature-dependent heat capacities greater than T2/K2. CP,m(H2,g)=22.66+0.0438TK-1.0835x10-4T2K2J-K-1-mol-1 CP,m(N2,g)=30.81-0.01187TK+2.3968x10-5T2K2J-K-1.mol-1 CP,m(NH3,g)=29.29+0.01103TK+4.2446x10-5T2K2J-K-1.mol-1 H2(g) N2(g) NH3(g) So(J.mol-1 K-1) 130.7 191.6 192.8
Calculate 4G in two different ways for the dimerization of NO₂. The first method uses the Gibbs free energies of formation and the second method uses the equation 4G = AH-TAS. 2NO₂(g) → N₂O4(g) Starting with the natural variable equation of dH = TdS+Vdp, show that OH др T = V(1-aT)
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction C,H,(g) + H, (g) =2CH,(g) the standard change in Gibbs free energy is AG" = -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are Pc,H, = 0.450 bar, P, = 0.400 bar, and PCH, = 0.900 bar? AG = kJ/mol