To determine the spontaneity of a chemical reaction, the sign of AG rather than the sign of AS is generally used. This is because O (1) AG is always positive and AS may be positive or negative O (2) Free energy free and it is easier to understand than entropy. O (3) AG is always larger than AS O (4) none given Que

To determine the spontaneity of a chemical reaction, the sign of AG rather than the sign of AS is generally used. This is because O (1) AG is always positive and AS may be positive or negative O (2) Free energy free and it is easier to understand than entropy. O (3) AG is always larger than AS O (4) none given Que

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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Consider the reaction 2H₂S(g) + 30₂(g) 2H₂O(g) + 250₂(g) Based upon the stoichiometry of the reaction the sign of ASOrxn should be Using standard thermodynamic data (in the Chemistry References), calculate ASºrn at 25°C. ASOrxn J/K mol negative.
If ΔS ̊sys = -198.3 J/K, is the reaction spontaneous at 25 ̊C.
- Chapter 9 and 18 - Thermodynamics Exercise 18.36 Enhanced with Feedback and Hints Without doing any calculations, determine the sign of ASsys for each of the following chemical reactions. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help CH4(g) + 202(g)→ CO2(g) + 2H2O(1) 203(g) → 302(g) SO3(g) + H2O(1)→H2SO4(1) Mg(s) + Cl2 (g) → MgCl2 (s) ASsy greater than 0 ASy smaller than 0
Which substance would have the greatest standard molar entropy? A)H2O (l) B)Al (s) C)NO (g) D)He (g)
7. The decomposition of ammonium chloride to form ammonia and hydrogen chloride occurs NH,Cl→ NH3(e + HCle AH = 176 kJ according to the following reaction: a) Predict the sign of the entropy change, AS, for this reaction. Justify your answer. b) The value of AG° for the reaction is negative at high temperatures but positive at low temperatures. Explain.
Consider the following reaction at constant pressure. Use the information here to determine the value of AS surr at 298 K. Predict whether or not this reaction will be spontaneous at this temperature. N₂(g) +202(g) → 2NO₂(g) AHrxn = +88.4 kJ mol-1 ASsurr = +88.4J K-1 mol-1, reaction is spontaneous Assurr = -88.4J K-1 mol-1, reaction is spontaneous ASsurr = -88.4J K-1 mol-1, reaction is not spontaneous ASsurr = +297 J K-1 mol-1, reaction is spontaneous ⒸASsurr = -297J K-1 mol-1, reaction is not spontaneous
As a fuel, H2(g) produces only non-polluting H2O(g) when it burns. Moreover, itcombines with O2(g) in a fuel cell to provide electrical energy.a) Calculate ΔHosys, ΔSosys, and ΔGosys per mole of H2(g) at 298K. b) Is the spontaneity of this reaction dependent on T? c) At what temperature does the reaction become spontaneous?
Arrange Au(s), Al(s), and C(s) in order of increasing entropy. Assume the three solids are at the same temperature.
3.
2 For the synthesis of ammonia where AG = -33.3 kJ/mole, determine whether the reaction is spontaneous at 25 C with the following pressures: PN, = 1.0 atm, PH, = 3.0 atm, PNH, = 0.020 atm N2(8) + 3H2(g) = 2NH3(g)
Determine which of the following has the highest entropy: He(g) Ne(g) Ar(g) Kr(g)
Use the data to calculate the standard entropy change for the following reaction: 5. S°[Mt(s)] 43.2 J/K mol Mt(s) + ½ O2(g) → MtO(s) S°[O2(g)] = 305.1 J/K-mol S°[MtO(s)] 62.6 J/K mol a) -133.2 J/K b) -285.7 J/K c) 285.7 J/K d) 133.2 J/K