None Which one of the following constant pressure processes has AS> 0 when the process goes tocompletion?show work. don't(A) Ag (s) @ 100°C→ Ag (s) @ 85°Cgive Ai generatedsolution(B) Cl(aq) +Ag (aq) AgCl (s)(C) 2Na (s) + 2H2O(l) 2NaOH (aq) + H2(g)(D) 500 puzzle pieces are assembled into a completed puzzle(E) N2 (g) + 3H2 (g)2NH3 (g)

Entropy (S) is the measure of randomness of a system. Higher the disorder higher is the…

Answered: Which one of the following constant…

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 62QAP: Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the...

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Similar questions

Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.
What is a spontaneous reaction?
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
A process that is reactant-favored at equilibrium can never be spontaneous. This statement is (a) true (b) false
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
The equilibrium constant for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either H or S.
Initially, only A and B are present, each at 2.00 mol · L. What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units.
Are the following redox reactions spontaneous under standard conditions?(a) Zn(s) + Ni2+(aq)------>Zn2+(aq) + Ni(s)(b) Zn(s) + Ca2+(aq)--------->Zn2+(aq) + Ca(s)
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