What is A in the following reaction 2Fe^{3+}_ | vedclass

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(B) In the given redox reaction: $2Fe^{3+}_{(aq)} + Sn^{2+}_{(aq)} 	o 2Fe^{2+}_{(aq)} + A$.We must balance the charge and the atoms on both sides of

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$Sn^{4+}_{(aq)}$

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(B) In the given redox reaction: $2Fe^{3+}_{(aq)} + Sn^{2+}_{(aq)} 	o 2Fe^{2+}_{(aq)} + A$.We must balance the charge and the atoms on both sides of the equation.The total charge on the reactant side is $(2 	imes +3) + (+2) = +8$.The total charge on the product side is $(2 	imes +2) + 	ext{charge of } A = +4 + 	ext{charge of } A$.For the equation to be balanced,the total charge must be equal on both sides: $+8 = +4 + 	ext{charge of } A$,which means the charge of $A$ is $+4$.Additionally,the oxidation half-reaction is $Sn^{2+} 	o Sn^{4+} + 2e^-$,where $Sn^{2+}$ is oxidized to $Sn^{4+}$.Therefore,$A$ is $Sn^{4+}_{(aq)}$.

What is $A$ in the following reaction $2Fe^{3+}_{(aq)} + Sn^{2+}_{(aq)} \to 2Fe^{2+}_{(aq)} + A$?

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