# In the following reaction, how many grams of hydrogen, H_2, will be produced from 53.5 g of...

## Question:

In the following reaction, how many grams of hydrogen, H_2, will be produced from 53.5 g of aluminum, Al?

2Al + 3H_2SO_4 -> 3H_2 + Al_2(SO_4)_3

## Molar Mass:

In chemistry, molar mass is the total mass in grams of a given element or compound divided by the total amount of substance expressed in moles. For compounds, molar mass is equal to the sum of all the products of the standard atomic weight of the elements multiplied by the number of atoms present.

Based from the chemical equation, {eq}2 \ moles{/eq} of aluminum will produce {eq}3 \ moles{/eq} of hydrogen molecule.

From that, we can determine the mass of the hydrogen molecule by doing the following steps.

Converting {eq}53.5 \ g{/eq} of aluminum into moles:

Note that: {eq}Al \ (molar \ mass) = 27 \frac{g}{mol}{/eq}.

{eq}\large Al_{moles} = \frac{mass}{molar \ mass} = \frac{53.5 \ g}{27 \frac{g}{mol}} = 1.98 \ mol {/eq}

Since, {eq}2 \ moles{/eq} of aluminum will produce {eq}3 \ moles{/eq} of hydrogen molecule, by ratio, {eq}1.98 \ moles{/eq} of aluminum will produce:

{eq}\frac{1.98 \times 3}{2} = 2.97 \ moles {/eq} of {eq}H_2{/eq}.

Converting {eq}2.97 \ moles{/eq} into mass:

(Note that: {eq}H{/eq} (molar mass) = {eq}1 \frac{g}{mol}{/eq})

{eq}H_{2mass} = 2.97 \ moles \times (2 \times 1 \frac{g}{mol}) = 5.94 \ g {/eq}

From the equation {eq}53.5 \ g{/eq} of {eq}Al{/eq} will produce {eq}5.94 \ g{/eq} of {eq}H_2{/eq}.