# Given the reaction of 0.25 g of Al with HCl, how many liters of H_2 gas will be produced if the temperature is 40 C and the pressure is 1.15 atm?

## $2 A {l}_{\left(s\right)} + 6 H C {l}_{\left(a q\right)} \to 3 {H}_{2 \left(a q\right)} + 2 A l C {l}_{3 \left(a q\right)}$

Jan 18, 2017

Approx. $300 \cdot m L \text{ of dihydrogen}$

#### Explanation:

You have the stoichiometric equation. We work out the molar equivalence of aluminum metal,

$\text{Moles of Al}$ $=$ $\frac{0.25 \cdot g}{27.0 \cdot g \cdot m o {l}^{-} 1} = 9.26 \times {10}^{-} 3 \cdot m o l$

$\text{Moles of dihydrogen}$ $=$ $\frac{3}{2} \times 9.26 \times {10}^{-} 3 \cdot m o l = 0.0139 \cdot m o l$

And $V = \frac{n R T}{P}$, where $n = 0.0139 \cdot m o l$, so............

$\frac{0.0139 \cdot \cancel{m o l} \times 0.0821 \cdot L \cdot \cancel{a t m} \cdot \cancel{{K}^{-} 1} \cdot \cancel{m o {l}^{-} 1} \times 313 \cdot \cancel{K}}{1.15 \cdot \cancel{a t m}}$

=??L