posted this before but it was wrong, can't figure out the stoichiometry part, can someone explain step by step.

Acid precipitation dripping on limestone produces carbon dioxide by the following reaction: CaCO3(s) +24+ (aq) Ca+ (aq) + CO2(g) +H20(1) 18.5 mL of CO2 was produced at 25.0C and738.0 mm Hg. 1st attempt Part 1 (1 point) l See Periodic Table See Hint How many moles of CO2 were produced? mol Part 2 (1 point) See Hint How many milligrams of CaCO3 were consumed? mg