A cell must work to maintain a stable internal environment. It is also important for the environment around the cell to be stabl
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<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)
- <u>For nickel:</u>
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
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:
- <u>For aluminium:</u>
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
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.