How many millliters of 275 M H_2SO_4(aq) are needed to react completely with 58.5 g of BaO_2(s)?

Jul 7, 2016

Are you sure mean barium peroxide, $B a {O}_{2}$, and not barium oxide, $B a O$.

Explanation:

$B a {O}_{2} \left(s\right) + {H}_{2} S {O}_{4} \left(a q\right) \rightarrow B a S {O}_{4} \downarrow + {H}_{2} {O}_{2} \left(a q\right)$

This used to be used as an industrial method to make hydrogen peroxide.

So $\text{moles of barium peroxide}$ $=$ $\frac{58.5 \cdot g}{169.33 \cdot g \cdot m o {l}^{-} 1}$ $=$ $0.345 \cdot m o l$.

We need $1$ $\text{equiv}$ sulfuric acid.

If $0.275 \cdot m o l \cdot {L}^{-} 1$ sulfuric acid is available, we need $\frac{0.345 \cdot m o l}{0.275 \cdot m o l \cdot {L}^{-} 1} \times 1000 \cdot m L \cdot {L}^{-} 1$ $=$ $1255 \cdot m L$.