Do we need to know how to write redox equations under alkaline conditions? Also, would vcaa ask us to write equations for the reactions in fuel cells with alkaline, liquid, molten carbonate, or solid oxide electrolytes?
First bit - it's never been asked before, it's a safe no. However, it's actually pretty easy to do - first step to making an alkaline cell, simple balance it assuming it's in acidic conditions. Eg, let's say I have \(\ce{MnO4- + I- \to I2 + Mn^2+}\) Go through the steps:
Half-reaction 1: \(\ce{MnO4- \to Mn^2+}\)
1. Balance atoms that aren't oxygen or hydrogen: \(\ce{MnO4- \to Mn^2+}\)
2. Balance the oxygens by adding water: \(\ce{MnO4- \to Mn^2+ + 4H2O}\)
3. Balance the hydrogens by adding protons: \(\ce{MnO4- + 8H+ \to Mn^2+ + 4H2O}\)
4. Balance the charge: \(\ce{MnO4- + 8H+ + 5e- \to Mn^2+ + 4H2O}\)
Half-reaction 2: \(\ce{I- \to I2}\)
1. Balance atoms that aren't oxygen or hydrogen: \(\ce{2I- \to I2}\)
2. Balance the oxygens by adding water: \(\ce{2I- \to I2}\)
3. Balance the hydrogens by adding protons: \(\ce{2I- \to I2}\)
4. Balance the charge: \(\ce{2I- \to I2 + 2e-}\)
5. Combine the equations. I'm going to do 2*HR1 and 5*HR2:
\(\ce{2MnO4- + 16H+ + 10e- + 10I- \to 2Mn^2+ + 8H2O + 5I2 + 10e-}\)
Of course, the electrons cancel off:
\(\ce{2MnO4- + 16H+ + 10I- \to 2Mn^2+ + 8H2O + 5I2}\)
And you'd normally be done if this was acidic. For alkaline, now all you need to do is add the same amount of hydroxide to both sides of the equation as there are free protons:
\(\ce{2MnO4- + 16H+ + 10I- + 16OH- \to 2Mn^2+ + 8H2O + 5I2 + 16OH-}\)
NOTE: I've not really "added" anything new to the equation. Free hydroxide exists in all solutions of water, remember that water is in constant equilibrium with hydronium and hydroxide ions. I can add the hydroxide for the same reason I can add the acid.
And this is now in alkaline conditions! Do note that the protons and hydroxides on the same side should combine into water, and then cancel off any extra waters from the other side:
\(\ce{2MnO4- + 16H2O + 10I- \to 2Mn^2+ + 8H2O + 5I2 + 16OH-}\)
\(\ce{2MnO4- + 8H2O + 10I- \to 2Mn^2+ + 5I2 + 16OH-}\)
And you're done - alkaline condition redox reaction, with just one extra step of adding those hydroxides. Otherwise, see ArtyDreams for some good responses. Normally I wouldn't respond since they have, but I really wanted to showcase that the alkali version is not complicated, it's just 1 extra step