What quantity of water results from the combustion of a $0.5 \cdot g$ $0.5*g$ mass of dihydrogen gas?

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Answer 1 · 2016-08-15T18:31:10

Approx, $4.25 \cdot g$ $4.25*g$ .

First, we need a stoichiometrically balanced equation, i.e.

$H_2(g) + 1/2O_2(g) rarr H_2O(g)+Delta$

$"Moles of dihydrogen"$ $=$ $(0.5*g)/(2xx1.00794*g*mol^-1)=0.25*mol$

Given the $1:1$ stoichiometry, if $0.25*mol$ dihydrogen react, then $0.25*mol$ water result.

$"Mass of water"$ $=$ $0.25*cancel(mol)xx18.02*g*cancel(mol^-1)=??g$

How many grams of dioxygen were involved?

What quantity of water results from the combustion of a 0.5*g0.5⋅g0.5*g mass of dihydrogen gas?