Answer:
6.67 grams of hydrogen can be formed when 60 g of aluminum reacts with excess hydrochloric acid.
Step-by-step explanation:
The balanced reaction is:
2 Al + 6 HCl → Al₂Cl₆ + 3 H₂
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- Al: 2 moles
- HCl: 6 moles
- Al₂Cl₆: 1 mole
- H₂: 3 moles
Being the molar mass:
- Al: 27 g/mole
- HCl: 36.45 g/mole
- Al₂Cl₆: 266.7 g/mole
- H₂: 2 g/mole
By reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- Al: 2 moles* 27 g/mole= 54 grams
- HCl: 6 moles* 36.45 g/mole= 218.7 grams
- Al₂Cl₆: 1 mole* 266.7 g/mole= 266.7 grams
- H₂: 3* 2 g/mole= 6 grams
You can apply the following rule of three: if 54 grams of aluminum forms 6 grams of hydrogen, 60 grams of aluminum will form how much mass of hydrogen?
mass of hydrogen= 6.67 grams
6.67 grams of hydrogen can be formed when 60 g of aluminum reacts with excess hydrochloric acid.