In a Commercial Laboratory, the Acid in Sulfuric Acid Waste $\rarr$

In a commercial laboratory, the acid in sulfuric acid waste can be readily neutralized using finely ground limestone chips. The reaction is:
H₂SO₄(aq) + CaCO₃(s) $\rarr$ H₂O(l) + CO₂(g) + CaSO₄(s)
A large bath holds 1.00 × 10⁴ liters of solution, which is enough to fill 50 of the 2.00×10² liter drums. The acid content of the "neutralized"bath was determined to be 1.50 M in H₂SO₄. How many metric tons (1 metric ton = 1.000 × 10³ kg) of CaCO₃ would be the minimum amount to neutralize the acid in this bath?

A) 0.750 metric tons
B) 1.02 metric tons
C) 1.50 metric tons
D) 2.04 metric tons
E) 3.54 metric tons