Answer: The amount of hydrogen gas that could be produced by the chemical reaction is 0.122 grams
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)
Given mass of aluminium = 1.80 g
Molar mass of aluminium = 27 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of aluminium}=\frac{1.80g}{27g/mol}=0.066mol[/tex]
Given mass of sulfuric acid = 6.00 g
Molar mass of sulfuric acid = 98 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of sulfuric acid}=\frac{6.00g}{98g/mol}=0.061mol[/tex]
The given chemical equation follows:
[tex]2Al+3H_2SO_4\rightarrow Al_2(SO_4)_3+3H_2[/tex]
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 = [tex]\frac{2}{3}\times 0.061=0.0408mol[/tex] 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 = [tex]\frac{3}{3}\times 0.061=0.061moles[/tex] 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:
[tex]0.061mol=\frac{\text{Mass of hydrogen gas}}{2g/mol}\\\\\text{Mass of hydrogen gas}=(0.061mol\times 2g/mol)=0.122g[/tex]
Hence, the amount of hydrogen gas that could be produced by the chemical reaction is 0.122 grams
