<u>Answer:</u> The mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
 .....(1)
      .....(1)
Given mass of nickel = 14.8 g
Molar mass of nickel = 58.7 g/mol
Putting values in equation 1, we get:

For the given chemical reaction:

- <u>For nickel (II) oxide:</u>
By Stoichiometry of the reaction:
3 moles of nickel are produced from 3 moles of nickel (II) oxide
So, 0.252 moles of nickel will be produced from  of nickel (II) oxide
 of nickel (II) oxide
Now, calculating the mass of nickel (II) oxide by using equation 1:
Molar mass of nickel (II) oxide = 74.7 g/mol
Moles of nickel (II) oxide = 0.252 moles
Putting values in equation 1, we get:

By Stoichiometry of the reaction:
3 moles of nickel are produced from 2 moles of aluminium
So, 0.252 moles of nickel will be produced from  of aluminium
 of aluminium
Now, calculating the mass of aluminium by using equation 1:
Molar mass of aluminium = 27 g/mol
Moles of aluminium = 0.168 moles
Putting values in equation 1, we get:

Hence, the mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.