This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Hey HΓΈlΓΌwΓ₯rh, good to see you again. To determine if magnesium will displace aluminum ions, we need to calculate the standard cell potential (E^_cell) for the reaction. A positive E^_cell indicates a spontaneous reaction. Step 1: Identify the half-reactions and their standard potentials. The given standard reduction potentials are: For magnesium: Mg^2+(aq) + 2e^- Mg(s), E^_red = -2.375\,V For aluminum: Al^3+(aq) + 3e^- Al(s), E^_red = -1.660\,V Step 2: Determine the oxidation and reduction processes. For magnesium to displace aluminum ions, magnesium metal (Mg(s)) must be oxidized, and aluminum ions (Al^3+(aq)) must be reduced. The oxidation half-reaction for magnesium is the reverse of its reduction: Mg(s) Mg^2+(aq) + 2e^- The standard oxidation potential (E^_ox) is the negative of the standard reduction potential: E^_ox(Mg) = -(-2.375\,V) = +2.375\,V The reduction half-reaction for aluminum ions is already given: Al^3+(aq) + 3e^- Al(s), E^_red(Al) = -1.660\,V Step 3: Calculate the standard cell potential (E^_cell). The standard cell potential is the sum of the standard oxidation potential and the standard reduction potential: E^_cell = E^_ox(Mg) + E^_red(Al) E^_cell = (+2.375\,V) + (-1.660\,V) E^_cell = 2.375\,V - 1.660\,V E^_cell = +0.715\,V Step 4: Conclude based on the standard cell potential. Since the standard cell potential (E^_cell) is positive (+0.715\,V), the reaction is spontaneous under standard conditions. This means magnesium will displace aluminum ions from the solution. The overall balanced reaction is: 3Mg(s) + 2Al^3+(aq) 3Mg^2+(aq) + 2Al(s) Magnesium will displace aluminum ions from the solution. Yes, Magnesium will displace Aluminum ions. Send me the next one πΈ