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Chapter 18: Problem 27

Which of the following reactions is (are) spontaneous at standard conditions? (a) \(2 \mathrm{NO}_{3}^{-}(a q)+8 \mathrm{H}^{+}(a q)+6 \mathrm{Cl}^{-}(a q) \longrightarrow\) \(2 \mathrm{NO}(g)+4 \mathrm{H}_{2} \mathrm{O}+3 \mathrm{Cl}_{2}(g)\) (b) \(\mathrm{O}_{2}(g)+4 \mathrm{H}^{+}(a q)+4 \mathrm{Cl}^{-}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{Cl}_{2}(g)\) (c) \(3 \mathrm{Fe}(s)+2 \mathrm{AuCl}_{4}^{-}(a q) \longrightarrow 2 \mathrm{Au}(s)+8 \mathrm{Cl}^{-}(a q)+3 \mathrm{Fe}^{2+}(a q)\)

Short Answer

Expert verified
Provide the calculated ∆G° values for each reaction to support your answer.

Step by step solution

01

(a) Calculate ∆G° for reaction (a)

Using the standard Gibbs free energy values from a table, find the ∆G° values for the reactants and products of reaction (a). Subtract the sum of the reactant ∆G° values from the sum of the product ∆G° values to find the ∆G° for the reaction.
02

(b) Calculate ∆G° for reaction (b)

Repeat step (a) for the reactants and products of reaction (b).
03

(c) Calculate ∆G° for reaction (c)

Repeat step (a) for the reactants and products of reaction (c). Step 2: Determine if each reaction is spontaneous
04

(a) Determine spontaneity for reaction (a)

If the calculated ∆G° for reaction (a) is negative, then the reaction is spontaneous. If the ∆G° is positive or zero, the reaction is non-spontaneous or reaches equilibrium, respectively.
05

(b) Determine spontaneity for reaction (b)

Repeat step (a) for the calculated ∆G° of reaction (b).
06

(c) Determine spontaneity for reaction (c)

Repeat step (a) for the calculated ∆G° of reaction (c). Step 3: Conclusion
07

Conclusion

Based on the calculated ∆G° values and the spontaneity determinations, list which of the reactions (a), (b), and (c) are spontaneous at standard conditions.

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Most popular questions from this chapter

A solution containing a metal ion \(\left(M^{2+}(a q)\right)\) is electrolyzed by a current of \(7.8\) A. After \(15.5\) minutes, \(2.39 \mathrm{~g}\) of the metal is plated out. (a) How many coulombs are supplied by the battery? (b) What is the metal? (Assume \(100 \%\) efficiency.)

Consider a voltaic cell in which the following reaction occurs. $$ \mathrm{Zn}(s)+\mathrm{Sn}^{2+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Sn}(s) $$ (a) Calculate \(E^{\circ}\) for the cell. (b) When the cell operates, what happens to the concentration of \(\mathrm{Zn}^{2+}\) ? The concentration of \(\mathrm{Sn}^{2+}\) ? (c) When the cell voltage drops to zero, what is the ratio of the concentration of \(\mathrm{Zn}^{2+}\) to that of \(\mathrm{Sn}^{2+}\) ? (d) If the concentration of both cations is \(1.0 \mathrm{M}\) originally, what are the concentrations when the voltage drops to zero?

Which of the following reactions is (are) spontaneous at standard conditions? (a) \(\mathrm{Zn}(s)+2 \mathrm{Fe}^{3+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+2 \mathrm{Fe}^{2+}(a q)\) (b) \(\mathrm{Cu}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{H}_{2}(g)\) (c) \(2 \mathrm{Br}^{-}(a q)+\mathrm{I}_{2}(s) \longrightarrow \mathrm{Br}_{2}(l)+2 \mathrm{I}^{-}(a q)\)

Consider a cell in which the reaction is $$ 2 \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q) \longrightarrow 2 \mathrm{Ag}^{+}(a q)+\mathrm{Cu}(s) $$ (a) Calculate \(E^{\circ}\) for this cell. (b) Chloride ions are added to the \(\mathrm{Ag} \mid \mathrm{Ag}^{+}\) half- cell to precipitate \(\mathrm{AgCl}\). The measured voltage is \(+0.060 \mathrm{~V}\). Taking \(\left[\mathrm{Cu}^{2+}\right]=1.0 \mathrm{M}\), calculate \(\left[\mathrm{Ag}^{+}\right]\). (c) Taking \(\left[\mathrm{Cl}^{-}\right]\) in \((\mathrm{b})\) to be \(0.10 M\), calculate \(K_{\text {sp }}\) of \(\mathrm{AgCl}\).

Which of the following species will be oxidized by \(1 \mathrm{MHCl}\) ? (a) \(\mathrm{Au}\) (b) \(\mathrm{Mg}\) (c) Cu (d) \(\mathrm{F}^{-}\)
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