In 1901, thomas edison invented the nickel-iron battery. the following reaction takes place in the battery. fe(s) + 2 nio(oh)(s) + 2 h2o(l) fe(oh)2(s) + 2 ni(oh)2(aq) how many mole of fe(oh)2, is produced when 6.00 mol fe and 8.45 mol nio(oh) react?

There is 4.225 moles Fe(OH)2 produced.

Explanation:

Step 1: Data given

Number of moles Fe = 6.00 moles

Moles of NiO(OH) = 8.45 moles

Molar mass Fe = 55.85 g/mol

Molar mass NiO(OH) = 91.70 g/mol

Step 2: The balanced equation

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

Step 3: Calculate limiting reactant

For 1 mol Fe we need 2 moles NiO(OH) and 2 moles H2O to produce 1 mol Fe(OH)2 and 2 moles Ni(OH)2

NiO(OH) is the limiting reactant. It will completely be consumed (8.45 moles). Fe is in excess. There will react 8.45 / 2 = 4.225 moles Fe.

There will remain 6.00 - 4.225 moles = 1.775 moles Fe

Step 4: Calculate moles of Fe(OH)2

For 1 mol Fe we need 2 moles NiO(OH) and 2 moles H2O to produce 1 mol Fe(OH)2 and 2 moles Ni(OH)2

For 8.45 moles NiO(OH) we'll have 8.45 /2 = 4.225 moles Fe(OH)2 produced.

There is 4.225 moles Fe(OH)2 produced.

imma come back to you hold on

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be