Wheste ion stofanc. Using standard thermodynamic data, calculate the following for rubidiumperchlorate in water:i. AGsoln at 25.0 °Cii. KSp at 25.0 °Ciii. The temperature at which the dissolution of rubidium perchlorate becomesspontaneous. Is this an upper or lower limit to spontaneity?iv. Can rubidium perchlorate be made to spontaneously dissolve in water at101.3 kPa? Explain.

The reactions are written as follows:

Answered: Wheste ion stofan c. Using standard…

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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Calculate the change in entropy of a 1kg of He gas at the normal boiling point of He when it all condenses isothermally to 1L of liquid He. TABLE 17.4 Heats of Fusion and Vaporization Normal Melting Polnt Normal Bolling Heat of Heat of Polnt Fuslon, L4 (J/kg) Vaportzation, I (J/kg) Substance K K "C Helium 4.216 -268.93 20.9 x 10' Hydrogen 13.84 -259.31 58.6 x 10 20.26 -252.89 452 x 10 Nitrogen 63.18 -209.97 25.5 x 10 77.34 -195.8 201 x 10 Oxygen 54.36 -218.79 13.8 x 10 90.18 -183.0 213 х 10° Elhanol 854 x 10 199 -114 104.2 x 10 351 78 Mercury 234 -39 11.8 x 10 630 357 272 x 10 Water 273.15 0.00 334 x 10 373.15 100.00 2256 x 10 Sulfur 392 119 38.1 x 10 717.75 444,60 326 x 10 Lead 600.5 327.3 24.5 x 10 2023 1750 871 x 10 Antimony 903.65 630.50 165 x 10 1713 1440 S61 x 10 Silver 1233.95 960.80 88.3 x 10 2466 2193 2336 x 10 Gold 1336.15 1063.00 64.5 x 10 2933 2660 1578 x 10' Соррer 1356 1083 134 x 10 1460 1187 5069 x 10 "A pressure in excess of 25 atmospheres is required to make helium…
Which of the following statements concerning entropy change is/are true? 1. For a spontaneous process, AS>q/T 2. For a spontaneous process, AS=entropy created+q/T 3. For an equilibrium process (such as a phase change), AS=q/T
Calculate the standard entropy change for the formation of 1.0 mol of the following compounds from the elements at 25 °C. a. C2H4 (g) Use the following data: J K. mol C2H4 (g) C(s, graphite) H2 (g) 219.36 5.6 130.7 A,S° = J/K-mol-rxn b. MgCO3 (s) Use the following data: J S° K- mol MgCO3 (s) 65.84 Mg(s) C(s, graphite) 02 (g) 32.67 5.6 205.07 A,S° = J/K-mol-rxn
11. Which of the following statements concerning entropy change is/are true? 1. For a reversible process, ΔS < 0.2. For a spontaneous process ΔSUniverse > 0.3. For a reversible process, such as a phase change, ΔS = qrev/T.
9
17. The acid HB ionizes 2.50 percent in a 0.600 M HB solution to reach equilibrium understandard state according to the reaction: HB(aq) + H2O(l) → H3O+(aq) + B-(aq) + 1.20 kJ . Determine entropy change for the ionization of HB under standard state.
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c. In the reaction between hydrogen gas and chlorine gas to give hydrogen chloride gas spontaneous, under standard conditions? Predict the spontaneity based on the calculated values of enthalpy change, standard entropy, and AS°universe. H2ie + Cle) 2H€I, (3). Standard entropy values, S° in J/mol-K: H 130.7; Cla = 223.0; HCI = 186.8 2(g) 2(g) Standard enthalpy of formation, AHf", for HCl -92.3 kJ/mol
1. The heat capacity at 1 atm. pressure of solid magnesium in the temperature range from 0 °C to 560 °C, is given by the expression: C, = 6.20 + 1.33 x 103 T+ 6.78 x 10* T² Cal. deg." g. atom. What is the increase of entropy per g. atom, for an increase of temperature from 300 K to 800 K at 1 atm. pressure?
The reaction 2 C4H10(g) + 13O2(g) - has AG° = -5407 kJ. Determine the value of AG°, for C4H10(8). 8 CO2lg) + 10 H20(g) Standard Free Energies of Formation of Typical Substances at 298.15 K TABLE 18.2 Substance Substance Substance AG? (kJ mol ') AG? (kJ mol-") AG? (kJ mol ) Agt) CaO6) -604.2 K,SO,G) -1316.4 AgC6) -109.7 Ca(OH),() -896.76 N,() Al() 0.00 CaSO) NH,(g) NH.CI() -1320.3 -16.7 ALĻO,6) C) (graphite) COO Co,( -1576.4 CaSO, H,OG) -1435.2 - 203.9 CaSO,2H,0G) -1795.7 NO(g) + 86.69 NO,(g) N,O) N,0, -137.3 +51.84 -394.4 Fe() +103.6 CH( -50.79 Fe,O,6) -741.0 +98.28 CH,A(g) -58.6 Na() CH,OH() -166.2 H,0(g) -228.6 Na,CO,() -1048 CO(NH)l) -197.2 -237.2 NaHCO,6) -851.9 CO(NH)(ag) C,H,(g -203.8 HCI -95.27 NaC) -384.0 +209 HNO,) -79.91 NaOH) -382 +68.12 H,SO() -689.9 Na,SO.) -1266.8 HC,H,0,(/) Hg(/) Hg(g) -32.9 -392.5 C,H,OH() -174.8 PbO) -189.3 +17.3 +31.8 Ca(o) K() SO;(g) -300.4 Ca00,() -1128.8 KCI) -408.3 -370.4 CaC,6) -750.2 i kJ e Textbook and Media Choose the value of K, for the…
For the reaction delta H° = 98.8 kJ/mol and delta S° =141.5 J/(mol*K). 3H2 (g) +Fe2O2(s) →2Fe(s) +3H2O(g) (19) Over what temperature range (if any) is the reaction spontaneous?
Calculate ∆G° for the reaction of iron(III) oxide with carbon monoxide to give elemental iron and carbon dioxide.Use data in the table below:

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