By titration, 20.4 ml of aqueous h2so4 neutralized 23.3 ml of 0.0336 m lioh solution. what was the molarity of the aqueous acid solution?

The balanced equation for the neutralisation reaction is as follows
2LiOH + H₂SO₄ ---> Li₂SO₄ + 2H₂O
stoichiometry of LiOH to H₂SO₄ is 2:1
number of moles of LiOH moles reacted - 0.0336 mol/L x 0.0233 L = 7.83 x 10⁻⁴ mol
if 2 mol of LiOH reacts with 1 mol of H₂SO₄ 
then 7.83 x 10⁻⁴ mol of LiOH reacts with - 7.83 x 10⁻⁴ /2 mol = 3.92 x 10⁻⁴ mol of H₂SO₄
if 20.4 mL contains - 3.92 x 10⁻⁴ mol of H₂SO₄
then 1000 mL contains - 3.92 x 10⁻⁴ mol / 20.4 mL x 1000 mL / L = 0.0192 mol/L
molarity of H₂SO₄ solution - 0.0192 M

Elias is almost correct. he just got it backwards.the correct answer is that it demonstrates elastic potential energy transforming into kinetic energy.