contestada

For which of the following reactions is [tex]\Delta H^o_{rxn}[/tex] equal to [tex]\Delta H^o_f[/tex] of the product(s)?
1. [tex]C(s,graphite)+ O_2(g) \rightarrow CO_2(g)[/tex]
2. [tex]Na(s)+12 Cl_2(l) \rightarrow NaCl(s)[/tex]
3. [tex]2Na(s)+ Cl_(g) \rightarrow 2NaCl(s)[/tex]
4. [tex]CO(g) + 12O_2(g) \rightarrow CO_2(g)[/tex]
5. [tex]CaCO_3(g) \rightarrow CaO+ CO_2(g)[/tex]
6. [tex]Na(s) + 12Cl_2(g) \rightarrow NaCl(s)[/tex]

Respuesta :

IthaloAbreu

Answer:

1 and 6.

Explanation:

The enthalpy of reaction (ΔH°rxn) can be calculated by the enthalpy of the formation (H°f) of the components:

ΔH°rxn = ∑n*H°fproducts - ∑n*H°freactants, where n is the number of the moles of the stoichiometric reaction.

So, if ∑n*H°freactants = 0, ΔH°rxn = ∑n*H°fproducts = ΔH°f of the products.

H°f = 0 if the compound is formed by only one element and it is in the ambiental conditions phase. In this case:

H°f of C(s, graphite) = 0

H°f of O₂(g) = 0

H°f of Na(s) = 0

H°f of Cl₂(g) = 0

Thus, it happens only for reactions 1 and 6.

Otras preguntas