Identify the correct set-up. How many moles of aluminum oxide would form if 25.0 g of aluminum react completely given the following chemical reaction: 4Al + 3O₂ → 2Al₂O₃?

Option 1. 25g Al x 1mol Al/26.982g Al x 2mol Al₂O₃/ 4mol Al

Explanation:

The equation for the reaction is given below:

4Al + 3O₂ → 2Al₂O₃

Molar Mass of Al = 26.982g/mol

Mass of Al = 25g

The number of mole in 25g of Al can be expressed as:

25g of Al = 25g x 1 mol / 26.982g

From the balanced equation above,

4 mol of Al produced 2 moles of Al₂O₃.

Therefore, 25g of Al (25g x 1 mol / 26.982g) will produce =

25g Al x 1mol Al/26.982g Al x 2mol Al₂O₃/ 4mol Al

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.