Use the following steps to balance the redox reaction using half-reactions.
Zn(s) + Fe3+ → Zn2+ + Fe(s) (unbalanced)

a. Write balanced oxidation and reduction half-reactions. Indicate which is the
oxidation reaction and which is the reduction reaction.

b. Balance the charge in the two half reactions by multiplying the half-reactions by correct multiplication factors.

c. Add the equations and simplify to get the balanced equation.

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

l dont know l am s sorry

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer

answer: i dont know the answer but this might

explanation:

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