Question

Calculate the volume of H2 that will be produced from the complete consumption of 10.8 g Zn in excess 0.100 M HCl (P = 724 torr, T = 20.5 °C).? A. 8.35 L B.1.65×10-2 L C.4.18 L D.0.292 L E.5.49×10-3 L

Answer 1

I make it `C...`

Explanation:

We address the equation...

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

And thus the dihydrogen is EQUIMOLAR with the moles of zinc...

`"Moles of Zn"=(10.8*g)/(65.4*g*mol^-1)=0.165*mol.`

And thus `0.165*mol` of dihydrogen are evolved...

And we solve the ideal gas equation with the given conditions...

`V=(nRT)/P=(0.165*molxx0.0821*(L*atm)/(K*mol)xx293.65*K)/((724*mm*Hg)/(760*mm*Hg*atm))`

`=??*L`