Nickel-Iron Battery

Chemistry

2 answers:

tatuchka [14]3 years ago

8 0

The answer is: 4.00 mol of Fe(OH)2 is produced.

Balanced chemical reaction:

Fe(s) + 2NiO(OH)(s) + 2H₂O(l) → Fe(OH)₂(s) + 2Ni(OH)₂(aq).

n(Fe) = 5.00 mol; amount of iron.

n(NiO(OH)) = 8.00 mol; amount of nickel oxide hydroxide, limiting reactant.

From chemical reaction: n(NiO(OH)) : n(Fe(OH)₂) = 2 : 1.

n(Fe(OH)₂) = 8 mol ÷ 2.

n(Fe(OH)₂) = 4 mol; amount of iron(II) hydroxide.

irina1246 [14]3 years ago

6 0

Answer:

4.0 moles of Fe(OH)₂.

Explanation:

It is a stichiometry problem.

The balanced equation: <em>Fe + 2NiO(OH) + 2H₂O → Fe(OH)₂ + 2Ni(OH)₂</em>,

It is clear that 1.0 mole of Fe reacts with 2.0 moles of NiO(OH) and 2.0 moles of H₂O to produce 1.0 mole of Fe(OH)₂ and 2.0 moles of Ni(OH)₂.

The given data: <em>5.00 moles of Fe reacts with 8.00 mol of NiO(OH)</em>.

From the stichiometry; 4.0 moles of Fe (1.0 mole will be in excess) reacts completely with 8.0 moles of NiO(OH) and produce 4.0 moles of Fe(OH)₂.

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