When hydrogen peroxide decomposes, what mass of hydrogen peroxide is needed in solution to produce 1.6g of oxygen gas?

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When hydrogen peroxide decomposes, what mass of hydrogen peroxide is needed in solution to produce 1.6g of oxygen gas?

please answer quickly!!!

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Answer 1 · 2018-01-30T17:26:06

We need a stoichiometric equation....and we need approx. $3.5 \cdot g$ $3.5*g$

Explanation:

$H_{2} O_{2} (l) M n O_{2} - -- \to H_{2} O (l) + \frac{1}{2} O_{2} (g) ↑ ⏐ ⏐ ⏐$ $H_2O_2(l) stackrel(MnO_2)rarrH_2O(l)+1/2O_2(g)uarr$

This is in fact a disproportionation reaction...

$Moles of dioxygen = \frac{1.60 \cdot g}{32.00 \cdot g \cdot m o l^{- 1}} = 0.050 \cdot m o l$ $"Moles of dioxygen"=(1.60*g)/(32.00*g*mol^-1)=0.050*mol$

....and given the stoichiometry, we need $0.10 \cdot m o l$ $0.10*mol$ hydrogen peroxide....a molar quantity of $0.10 \cdot m o l \times 34.01 \cdot g \cdot m o l^{- 1} = ? ? g$ $0.10*molxx34.01*g*mol^-1=??g$

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When hydrogen peroxide decomposes, what mass of hydrogen peroxide is needed in solution to produce 1.6g of oxygen gas?

please answer quickly!!!

1 Answer

Explanation:

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