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Unformatted text preview: In order for a redox reaction to occur spontaneously… • The more active metal (higher) is oxidized • The less active metal (lower) is reduced The opposite can occur, but will require energy Practice: Write the balanced, spontaneous redox reactions between the following pairs of metals and their ions. 1. Mn (s)/Mn 2+ (aq) and Ni (s)/Ni 2+ (aq) 2. Fe (s)/Fe 3+ (aq) and Pb (s)/ Pb 4+ (aq) 3. Au (s)/Au 3+ (aq) and Sn (s)/Sn 2+ (aq) Conclusions • Not all redox reactions will occur spontaneously • Use the activity series (table J) to predict spontaneity ▫ Metals towards the top need to be oxidized ▫ Metals towards the bottom need to be reduced • Non-spontaneous redox reactions can occur, but require energy to do so...
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