31 Electrochemistry1

31 Electrochemistry1 - What do you predict? A) Silver metal...

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1 What do you predict? A) Silver metal will dissolve in a salt solution of copper nitrate. B) Copper metal will dissolve in a salt solution of silver nitrate. C) Both (A) and (B) will happen because salt solutions are corrosive. D) Neither (A) nor (B) will happen because metals are stable. 2 B) Copper dissolves in a salt solution of silver nitrate. Cu(s) + 2Ag + (aq) Cu 2+ (aq) + 2Ag(s)
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3 Why does this happen? The free energy decreases! Means its exothermic or the entropy increases Entropy probably deceases because 2 ions in solution go to 1! So reaction would have to be exothermic. 2 silver atoms are more strongly bound in the metal lattice than 1 copper atom. Compare enthalpies of fusion Cu 13.1 kJ/mol Ag 11.3 kJ/mol X 2 Cu(s) + 2Ag + (aq) Cu 2+ (aq) + 2Ag(s) 4 What type of a reaction is this? Notice electrons are transferred from copper atoms to silver atoms. Electron transfer reaction Oxidation – reduction reaction (aka redox) Electrochemical reaction Note the charge must be balanced to conserve electrons. MSJ Ch 19 Electrochemistry, pp. 920 – 976 Review MSJ Ch 5, sections 3 & 4 oxidation numbers Cu(s) + 2Ag + (aq) Cu 2+ (aq) + 2Ag(s)
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5 Redox reactions can be described by half reactions Oxidation half reaction is the loss of electrons. Cu(s) Cu 2+ (aq) + 2e Reduction half reaction is the gain of electrons.
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31 Electrochemistry1 - What do you predict? A) Silver metal...

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