an excess of aluminum foil is allowed to react with 225 ml of hcl that contains 18.0% hcl by mass what is mass of h2 is produced

Complete question is;

An excess of aluminum foil is allowed to react with 225 ml of an aqueous solution of HCl (d=1.088 g/ml) that contains 18% HCl by mass. what mass of H2(g) is produced?

1.218 g

Explanation:

We are given d_HCL = 1.088 g/ml

Converting to g/L gives;

d = 1.088 × 1000 = 1088 g/L

Now, we are told the solution contains 18% HCl by mass.

Thus;

d = 1088 × 18%

d = 195.84 g/L

Now, molar mass of HCl is 36.46 g/mol

Thus, molar concentration is;

M = 195.84/36.46

M = 5.37 mol/L

We are told the volume of HCl used was 225 ml or 0.225 L

Thus, number of moles used is;

n = 5.37 × 0.225

n = 1.208

The balanced reaction equation of the aluminum foil and HCl is;

2Al + 3HCl = 2AlCl3 + 3H2

Number of moles of H2 produced will be; n1 = 1.208/2 = 0.604 moles

Molar mass of H2 is 2.016 g/mol

Thus, mass of H2 produced = 0.604 × 2.016 = 1.218 g

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