Question

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

please answer quickly!!!

Answer 1

We need a stoichiometric equation....and we need approx. `3.5*g`

Explanation:

`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"=(1.60*g)/(32.00*g*mol^-1)=0.050*mol`

....and given the stoichiometry, we need `0.10*mol` hydrogen peroxide....a molar quantity of `0.10*molxx34.01*g*mol^-1=??g`