Question

Given: 2Al + 6HCl → 2AlCl3 + 3H2
If the chemical reaction produces 129 grams of AlCl3, how many grams of H2 are also produced?
A. 1.22
B. 2.92
C. 3.02
D. 3.65

Answer 1

the correct answer is B

Answer 2

2.92 grams of $H_2$ are also produced.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$      .....(1)

For $AlCl_3$

Given mass of $AlCl_3$ = 129 g

Molar mass of $AlCl_3$ = 133 g/mol

Putting values in equation 1, we get:

$\text{Moles of titanium}=\frac{129g}{133g/mol}=0.970mol$

The chemical equation for the reaction of aluminium and HCl follows:

$2Al+6HCl\rightarrow 2AlCl_3+3H_2$

By Stoichiometry of the reaction:

For 2 moles of $AlCl_3$ = 3 moles of hydrogen are produced

So, 0.970 moles of  $AlCl_3$ = $\frac{3}{2}\times 0.970=1.45mol$ of hydrogen

$1.45mol=\frac{\text{Mass of hydrogen}}{2g/mol}\\\\\text{Mass of hydrogen}=2.92g$

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