What is the maximum volume of hydrogen that can be liberated when 1.2 moles of zinc are added to excess dilute hydrochloride acid at room temperature and pressure?
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Would it not be approx. #30.5*L#?
We address the stoichiometric equation...
#Zn(s) + 2HCl(aq) rarr ZnCl_2(aq) +H_2(g)uarr#
And thus one equivalent of dihydrogen gas is produced by one equiv of zinc metal....
Here, we used #1.2*mol# of zinc metal reductant...and therefore we gets #1.2*mol# dihydrogen gas. And depending on your syllabus (and these days they are all over the place), one mole of gas occupies #22.4*dm^3# at #0# #""^@C#, or #25.4*dm^3# at #298# #K#...and so with the second definition, we take the product...
#25.4*dm^3*mol^-1xx1.20*mol=??L#
The balanced chemical reaction would be
#"Zn"+color(red)(2)"HCl"->"ZnCl"_2+"H"_2#
#=>color(blue)(1"mol")"Zn"+color(blue)(2"mol")"HCl"->color(blue)(1"mol")"ZnCl"_2+color(blue)(1"mol")"H"_2#
That means 1 mol Zn will yield 1 mol #"H"_2#. So, 1.2 mol Zn will yield 1.2 mol #"H"_2#.
1.2 × molar volume = 1.2 × 22.4
= 26.88 litres
