Determine the enthalpy change for the decomposition of calcium carbonate. caco₃(s) --> cao(s) + co₂(g) given the thermochemical equations below:
ca(oh)₂(s) --> cao(s) + h₂o(l); enthalpy reaction = 65.2 kj/mol
ca(oh)₂(s) + co₂(g) --> caco₃(s) + h₂o(l); enthalpy reaction = -113.8 kj/mol
c(s) + o₂(g) --> co₂(g); enthalpy of reation = -393.5 kj/mol
2ca(s) + o₂(g) --> 2cao(s); enthalpy of reaction = -1270.2 kj/mol

a. 1711.7 kj/mol rxn
b. 441 kj/mol rxn
c. 179 kj/mol rxn
d. 48 kj/mol rxn
e. 345.5 kj. mol rxn

c. 179 kJ/mol

Explanation:

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to Hess’s law, the chemical equation can be treated as algebraic expressions and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

Given:

      (1)

      (2)

      (3)

     (4)

On subtracting eq (1) from eq (2) we have:

-

Hence the enthalpy change for the raection is 179.0 kJ/mol.

ca has a crystalline lattice with positive ions (since it is a metal, metals are positively charged) and electrons flow freely in its structure since the ca atoms have a large nuclear radius so the electrons are not tightly held, therefore the electrons can flow freely since they are not being highly attracted by the nucleus. moreover, one of the properties of metals are that they are conductors of electricity, thus proving ca is the element.