What volume of #20%(w/w)# #"hydrochloric acid"# are need to oxidize a mass of #130*g# #"zinc metal"#?

1 Answer
Apr 15, 2017

Answer:

#Zn(s) +2HCl(aq) rarr ZnCl_2(aq) + H_2(g)uarr#

Explanation:

Now it is a fact that #20%(w/w)# #HCl# has a molar concentration of #6.0*mol*L^-1#. To calculate this you should have been given more details in the question.

We require a TWICE molar quantity with respect to the moles of zinc.

#"Moles of zinc"=(130*g)/(65.4*g*mol^-1)=2.0*mol#

And thus we need #1/3*L# #HCl(aq)# for stoichiometric equivalence.