a) Consider the sparingly soluble salt silver bromide. Write a balanced chemical equation showing the dissolution of silver bromide. b) Given the following information, provide the net reaction for the spontaneous reaction and determine the cell potential under standard conditions that would occur from these two half-reactions: Ag+(aq) + e- ⟶⟶ Ag(s) E°red = 0.80 V AgBr(s) + e- ⟶⟶ Ag(s) + Br-(aq) E°red = 0.07 V c) Calculate the equilibrium constant at 283 K (10.° C) for the spontaneous redox reaction you wrote in part b. d) Using only the information provided in this problem, calculate the solubility product constant of silver bromide at 10. °C. e) Is the dissolution of silver bromide at 10. °C thermodynamically favorable? Justify your response by determining ΔΔG°rxn at 10. °C, using only the information provided or determined in this problem.
a) Consider the sparingly soluble salt silver bromide. Write a balanced chemical equation showing the dissolution of silver bromide.
b) Given the following information, provide the net reaction for the spontaneous reaction and determine the cell potential under standard conditions that would occur from these two half-reactions:
Ag+(aq) + e- ⟶⟶ Ag(s) E°red = 0.80 V
AgBr(s) + e- ⟶⟶ Ag(s) + Br-(aq) E°red = 0.07 V
c) Calculate the equilibrium constant at 283 K (10.° C) for the spontaneous
d) Using only the information provided in this problem, calculate the solubility product constant of silver bromide at 10. °C.
e) Is the dissolution of silver bromide at 10. °C
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