Could someone please answer this chemistry question?

CaCO₃(s) + 2HNO₃(aq) → Ca(NO₃)₂(aq) + CO₂(g) + H₂O(ℓ)

Initial number of moles of CaCO₃ = (2.00 g) / (100 g/mol) = 0.0200 mol
Initial number of moles of HNO₃ = (0.1 mol/L) × (200/1000 L) = 0.0200 mol

According to the above equation, mole ratio CaCO₃ : HNO₃ = 1 : 2
If HNO₃ completely reacts, amount of CaCO₃ needed = (0.0200 mol) × (1/2) = 0.0100 mol < 0.0200 mol
Hence, CaCO₃ is in excess, and HNO₃ is the limiting reactant.
(A and B are false.)

According to the equation, mole ratio HNO₃ : Ca(NO₃)₂ = 2 : 1
Number of moles of HNO₃ reacted = 0.0200 mol
Number of moles of Ca(NO₃)₂ produced = (0.0200 mol) × (1/2) = 0.0100 mol
Mass of Ca(NO₃)₂ produced = (0.0100 mol) × (164 g/mol) = 1.64 g
(C is true.)

According to the equation, mole ratio HNO₃ : CO₂ = 2 : 1
Number of moles of HNO₃ reacted = 0.0200 mol
Number of moles of CO₂ produced = (0.0200 mol) × (1/2) = 0.0100 mol
Mass of Ca(NO₃)₂ produced = (0.0100 mol) × (24000 cm³/mol) = 240 cm³
(D is false.)

The answer: C. 1.64 g of calcium nitrate is produced by the reaction.