Iron (iii) oxide, also known as rust can be removed from iron by reacting it with hydrochloric acid to produce iron (iii) chloride and water. fe2o3 (s) + 6hcl (aq) > 2fecl3 + 3h2o (l) what mass of hydrogen chloride is required to react with 100 g of rust? a. 371g hcl b. 137g hcl c. 130g hcl d. 147g hcl

b. 137 g.

Explanation:

Fe₂O₃(s) + 6HCl(aq) → 2FeCl₃(s) + 3H₂O(l),

It is clear that 1.0 mole of Fe₂O₃ react with 6.0 mol of HCl to produce 2.0 moles of FeCl₃ and 3.0 moles of H₂O.

n = mass/molar mass = (100.0 g)/(159.69 g/mol) = 0.6262 mol.

Using cross multiplication:

1.0 mol of Fe₂O₃ react completely with → 6.0 mol of HCl, from stichiometry.

0.6262 mol of Fe₂O₃ produced with → ??? mol of HCl.

∴ The no. of moles of HCl = (6.0 mol)(0.6262 mol)/(1.0 mol) = 3.757 mol.

∴ The mass of HCl needed = no. of moles x molar mass = (3.757 mol)(36.46 g/mol) = 137.0 g.

So, the right choice is: b. 137 g.

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.