Answer: The amount of hydrogen gas that could be produced by the chemical reaction is 0.122 grams
Step-by-step explanation:
To calculate the number of moles, we use the equation:
.....(1)
Given mass of aluminium = 1.80 g
Molar mass of aluminium = 27 g/mol
Putting values in equation 1, we get:
Given mass of sulfuric acid = 6.00 g
Molar mass of sulfuric acid = 98 g/mol
Putting values in equation 1, we get:
The given chemical equation follows:
By Stoichiometry of the reaction:
3 moles of sulfuric acid reacts with 2 moles of aluminium
So, 0.061 moles of sulfuric acid will react with =
of aluminium
As, given amount of aluminium is more than the required amount. So, it is considered as an excess reagent.
Thus, sulfuric acid is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
3 moles of sulfuric acid produces 3 moles of hydrogen gas
So, 0.061 moles of sulfuric acid will produce =
of hydrogen gas
Now, calculating the mass of hydrogen gas from equation 1, we get:
Molar mass of hydrogen gas = 2 g/mol
Moles of hydrogen gas = 0.061 moles
Putting values in equation 1, we get:
Hence, the amount of hydrogen gas that could be produced by the chemical reaction is 0.122 grams