Question

1)

Why does balancing a redox equation use a different process than balancing other types of chemical equations?

Why does balancing a redox equation use a different process than balancing other types of chemical equations?

Because redox involves the movement of electrons, we have to make sure the oxidation numbers are the same on both sides of the reaction.

Because redox involves the movement of electrons, protons must be added to the appropriate side of the equation.

Because redox involves the movement of electrons, only the electrons need to be balanced on the two sides of the reaction, not the mass.

Because redox involves the movement of electrons, a redox equation has to balance the electron count on both sides.

2)

Balance each redox reaction occurring in acidic aqueous solution.

MnO4−(aq)+Al(s)→Mn2+(aq)+Al3+(aq)

3)

he equilibrium constant and the standard cell potential of an oxidation-reduction reaction related?

How are the equilibrium constant and the standard cell potential of an oxidation-reduction reaction related?

	Both are a function of the number of electrons transferred in the reaction.
	They are not related. The equilibrium constant derives from enthalpy while reduction potential only deals with charge.
	Both are a function of the standard change in Gibbs free energy.
	Both are related to the amount of work that can be done by a reaction on its surroundings.

Answer 1