How many liters are there in 0.500 g Hydrogen (H2)?

Answer

3.65 liters is the volume of H₂ produced in the reaction

Explanation:

2 Al(s) + 6 HCI (aq) → 2AICI₃ (aq) + 3 H₂ (g)

I'll convert the mass of Al to moles.

2.93 g . 1mol/26.98 g = 0.108 moles

Ratio is 2:3. 2 moles of Al can produce 3 moles of H₂

Then, 0.108 moles of Al would produce (0.108 .3)/ 2  = 0.163 moles of H₂ Let's apply the Ideal Gases Law to find out the produced volume, at STP.

STP is 1 atm as pressure and 273K as T°

1 atm . V = 0.163 mol . 0.082L.atm/mol.K . 273K

V = (0.163 mol . 0.082L.atm/mol.K . 273K) / 1atm

V = 3.65 L

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.