<h3>The following reactions is ΔH∘rxn equal to ΔH∘f of the product(s) : option a, b and d</h3><h3>Further explanation
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The change in enthalpy in the formation of 1 mole of the elements is called enthalpy of formation
The enthalpy of formation measured in standard conditions (25 ° C, 1 atm) is called the standard enthalpy of formation (ΔHf °)
Determination of the enthalpy of formation of a reaction can be through a calorimetric experiment, based on the principle of Hess's Law, enthalpy of formation table, or from bond energy data
Delta H reaction (ΔH) is the amount of heat / heat change between the system and its environment
(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)
The value of ° H ° can be calculated from the change in enthalpy of standard formation:
∆H ° rxn = ∑n ∆Hf ° (product) - ∑n ∆Hf ° (reactants)
ΔH∘rxn = ΔH∘f of the product(s) if ∆Hf ° (reactants) = 0
<em>The elements in standard conditions are not included in the enthalpy calculations because the enthalpy of those elements under the standard conditions is </em><em>zero.</em>
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a.ΔH°rxn = ∆Hf ° CO₂(∆Hf °C and ∆Hf °O₂ =0)
b.ΔH°rxn = ∆Hf ° LiCl(∆Hf °Li and ∆Hf °Cl₂=0)
c.ΔH°rxn = ∆Hf ° LiCl- 12∆Hf° Cl₂
d. ΔH°rxn = 2∆Hf °LiCl (∆Hf °Li and ∆Hf °Cl₂=0)
e. ΔH°rxn = ∆Hf °CO₂ - ∆Hf °CO
f. ΔH°rxn = ∆Hf °CO₂ + ∆Hf °BaO - ∆Hf ° BaCO₃
<h3>Learn more
</h3>
Delta H solution
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an exothermic reaction
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as endothermic or exothermic
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an exothermic dissolving process
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Keywords: Delta H reaction (ΔH), enthalpy of standard formation