Question

Aluminum reacts with sulfuric acid to form aluminum sulfate and hydrogen. What is the volume of hydrogen gas in liters (L) produced at 300 K and 1.0 atm pressure, when 5.4 g of aluminum and 50.0 mL of 5.0 M sulfuric acid are combined for the reaction?

Answer 1

we have to find the volume of Hydrogen gas in litre produced at 300K and 1 atm pressure when 5.4 g of aluminium and 50 ml of 5M sulphuric acid are combined for the reaction.

solution : 2Al + 3H₂SO₄ ⇒Al₂(SO₄)₃ + 3H₂

no of moles of Aluminium taken = 5.4/27 = 0.2

no of moles of sulphuric acid taken = 50ml × 5M/1000 = 0.25

we see 2 moles of Al reacts with 3 moles of sulphuric acid

so, 0.2 moles of Al reacts with 0.3 moles of sulphuric acid.

so, sulphuric acid is limited reagent.

now moles of H₂ formed = 3/3 × 0.25 = 0.25 [ as 3 moles of sulphuric acid form 3 moles of H₂ gas. ]

soz volume of H₂ gas formed = nRT/P [ from gas equation ]

= (0.25 × 0.082 × 300)/1 = 6.15 L

Therefore the volume of Hydrogen gas in litres is 6.15 L