When 10.9 g caco3 reacts with excess hydrochloric acid, as below, 3.79 g of co2 is produced. what is the percent yield of co2? do not type the units with your answer. caco3(s) + hcl(aq) => co2(g) + cacl2(aq) + h2o(l) (not balanced)

Yield of CO₂ = 79.1 %

Explanation:

This is the balanced reaction:

CaCO₃ (s) + 2HCl (aq) → CO₂ (g) + CaCl₂ (aq) + H₂O (l)

As the hydrochloric acid is in excess, the limiting reactant is the  CaCO₃.

Let's convert the mass to moles

10.9 g / 100.08 g/mol = 0.109 moles

Ratio is 1:1, so 0.109 moles of CaCO₃ will produce the same amount of CO₂.

Let's determine the mass

0.109 moles of CO₂ . 44 g/mol = 4.79 g

Now, we can determine the yield

(yeild produced / theoretical yield) . 100 =

(3.79 / 4.79) . 100 = 79.1%

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.