7 Simple Steps to Balancing Redox Reactions
<p>Cr2O72-+ 14H+ <strong>+ 6e- </strong>→ 2Cr3+ + 7H2O</p>
<p>This one’s a little tricky…</p>
<p>The overall charge of the reactants is +12, because of the 14H<strong>+</strong> and the one Cr2O72-</p>
<p>The overall charge of the products is +6 because of the 2Cr3+</p>
<p>Therefore, we add 6 electrons to the reactants so that both sides are +6</p>
<p>Fe2+ → Fe3+ <strong>+ e-</strong></p>
<p>The reactants are +2 and the products are +3, so the products need one electron</p>
<p>Notice how this reaction has electrons as <strong>products</strong> and the first one has electrons as <strong>reactants</strong></p>
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