b.The molar heat capacity of white tin (Snwhite) Varies with temperature as follows: 30 40 60 | 5.460 9.387 | 15.33 | 19.49 26.17 26.71 T/K 20 80 198 249 274 289 Cam/JK" 1.970 26.84 26.88 Calculate AG from grey/white tin transformation at 298 K (Given: Sywsm pry = 38.77 J K' AHsaey) Satwhae) = 2234 J]

b.The molar heat capacity of white tin (Snwhite) Varies with temperature as follows: 30 40 60 | 5.460 9.387 | 15.33 | 19.49 26.17 26.71 T/K 20 80 198 249 274 289 Cam/JK" 1.970 26.84 26.88 Calculate AG from grey/white tin transformation at 298 K (Given: Sywsm pry = 38.77 J K' AHsaey) Satwhae) = 2234 J]

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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X OWLV2 | Online tea Car note CAU EMAIL CANVAS Pirate Ship MYJSCC BLACKBOARD Vacancies | A..| Birmingham New NCOER C (Review Topics] [References] Use the References to access important values if needed for this question. For the reaction 2 H20(1) 2 H2(g) + O2(g) AG° = 462.5 kJ and AH° 571.6 kJ at 334 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 334 K. The entropy change for the reaction of 2.05 moles of H2O(1) at this temperature would be J/K. Submit Answer Retry Entire Group 9 more group attempts remaining DEC 3 étv MacBook Air
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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 =…
(a) 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.
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Compare DHm from (1) and (2) and comment.
Use the data given below to calculate AH° for the reaction, in units of kJ: A2B2 + B A2B3 Data: AH° (kJ) 2A,B3 + 11C → 4 AC, + 3 B2C AH°1 = -875 A2B2 + 5 C 2 AC2 + B2C AH°, = 807.2 B + 1/2 C 1/2 B2C AH°, = -250
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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
From the data in Table 2C.4 of the Resource section, calculate ΔrH⦵ and ΔrU⦵ at (i) 298 K, (ii) 478 K for the reaction C(graphite) + H2O(g) → CO(g) + H2(g). Assume all heat capacities to be constant over the temperature range of interest.