What is the minimum amount of 6.0 M H2SO4 necessary to produce 19.0 g of H2(g) according to the reaction?
2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)
2 answers
From given reaction equation, moles acid consumed = moles H2 produced = 19g/2g/mole = 9.5 moles acid = Molarity x Volume(L) = 6M x Vol(L) => 1.583 Liters of the Acid Solution
mols H2 gas = grams/molar mass = 19/2.0 = 9.5
mols H2SO4 needed = 9.5 since 1 mol H2SO4 = 1 mol H2 in the balanced equation.
M = mols/L or 6.0 = 9.5/L and L = 9.5/6.0 = 1.583 which I would round to 1.58 L.
mols H2SO4 needed = 9.5 since 1 mol H2SO4 = 1 mol H2 in the balanced equation.
M = mols/L or 6.0 = 9.5/L and L = 9.5/6.0 = 1.583 which I would round to 1.58 L.
1 answer