Limestone, caco3, reacts with hydrochloric acid to form calcium chloride, water and carbon dioxide

according to the following reaction:

caco3(s) + 2hcl(aq) → cacl2(aq) + h2o(l) + co2(g)

how many liters of co2 gas will be formed at 722 torr and 43.0°c by the reaction of 4.35 g limestone

with an excess of hydrochloric acid? assume 100% yield and that the gas is ideal.

answer:

explanation: caco3 + 2 hcl → cacl2 + h2o + co2

(29.0 g caco3) / (100.0875 g caco3/mol) = 0.289746 mol caco3

(15.0 g hcl) / (36.4611 g hcl/mol) = 0.411397 mol hcl

0.411397 mole hcl would react completely with 0.411397 x (1/2) = 0.2057 mol caco3 but there is more caco3 than that present, so caco3 is in excess and hcl is the limiting reactant.

(0.411397 mol hcl) x (1/2) x (110.9848 g cacl2/mol) = 22.8 g cacl2

(.289746 mol caco3 initially -   0.2057 mol caco3 reacted) x (100.0875 g caco3/mol) = 8.41 g caco3 left over

step-by-step explanation:

whole numbers, zero or greater

i believe it is c.) 1575 j.