Question

How many liters of H₂ gas would be produced when a 100.0 mL solution of 360.3 mM HCl is reacted with excess zinc as described by the reaction below? Assume a temperature of 28.6∘C and a pressure of 0.86 atm. Express your answer in liters using at least three significant figures.

Zn (s) + 2 HCl (aq) ⟶ ZnCl₂ (aq) + H₂ (g)

Answer 1

1.04L

Explanation

Zn(s) + 2HCl(aq) -------> ZnCl2(aq) + H2(g)

Stoichiometrically, 2moles of HCl gives 1 mole of H2

moles of HCl reacted = ( 0.3603mol/1000ml)×100ml = v0.03603mol

0.03603moles of HCl gives 0.03603moles of H2

Ideal gas equation is

PV = nRT

P = Pressure, 0.86atm

V = Volume

n = number of moles, 0.03603mol

R = gas constant, 0.082057L atm /mol K

T = Temperature, 28.6℃ = 301.75K

V = nRT/P

= 0.03603mol × 0.082057(L atm/mol K) × 301.75K / 0.86atm

= 1.04L