Energetic Definitions and Equations

The standard enthalpy change of formation of a compound is the enthalpy change which occurs when one mole of the compound is formed from its elements under standard conditions, and with everything in its standard state.

Does the following equation represent an enthalpy of formation reaction?

Mg_(g) + Cl_2(g)    →   MgCl_2(s)

The standard enthalpy change of formation of a compound is the enthalpy change which occurs when one mole of the compound is formed from its elements under standard conditions, and with everything in its standard state.

Does the following equation represent an enthalpy of formation reaction?

2C _{(s, graphite) +} O₂ + 4H_2(g) →  2CH₃OH_(l)

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one mole of the compound is burned completely in oxygen (in excess O₂) under standard conditions.

Does the following equation represent an enthalpy of combustion reaction?

CO (g)+ ½ O₂(g)⟶ CO₂(g)

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one mole of the compound is burned completely in oxygen (in excess O₂) under standard conditions.

Does the following equation represent a standard enthalpy of combustion reaction?

CH₃OH_(g)+ 3⁄2O_2(g)⟶CO_2(g)+2H₂O_(g)

Standard Enthalpy of Hydration, is the energy released when 1 mole of gaseous ions is completely hydrated in water to infinite dilution at standard conditions (298K and 1 atmospheric pressure).

            Identify the equation representing the enthalpy of hydration of nitrite ions.

Standard Enthalpy of Solution, ∆H^θ_solution is the energy change when 1 mole of a solute dissolves in solvent to form an infinitely dilute solution under standard conditions.

Does the following equation represent enthalpy of solution for Aluminium sulphate?

Al₂(SO₄ )_3(aq) + aq → 2Al_(aq)²⁺  +  3SO_4(aq)^3-

Standard Enthalpy change of Lattice formation (Lattice Energy) ∆H_L^θ    

is the energy released when 1 mole of an ionic solid is formed from its gaseous ions at standard conditions (298K and 1 atmospheric pressure).

            Identify the equation for lattice of formation for sodium oxide.

The standard atomisation enthalpy is the enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state at standard conditions.

Does the following equation represent an enthalpy of atomisation reaction?

½I₂ (s) → I (g)

The standard atomisation enthalpy is the enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state at standard conditions.

Does the following equation represent an enthalpy of atomisation reaction?

Cu (s) → Cu (g)

The 1^st Ionisation energy is

The energy absorbed when 1 mole of gaseous atoms is converted to gaseous ions with a single positive charge at standard conditions.

Does the following equation represent reaction for 1st ionisation energy.

K_(s) – 1e^-→ K_g)⁺

The 2^nd Ionisation energy is the energy absorbed to remove 1 mol of electrons from 1 mol of gaseous 1⁺ ions to form 1 mol of gaseous 2+ ions.

Does the following equation represent reaction for 2nd ionisation energy.

Fe_(g) – 2e^-→ Fe_(s)²⁺

The 1^st Electron affinity is the enthalpy change when 1 mole of gaseous atoms is converted to gaseous ions with a single negative charge.

Does the following equation represent reaction for 1^st Electron affinity.

S _(l) +1 e^- → S _(g)^-1

2^nd Electron Affinity is the enthalpy change when 1 mole of gaseous  1- ions gains 1 mol of electrons to be converted to 1 mol of gaseous 2- ions.

Does the following equation represent reaction for 2nd Electron affinity.

P^2- _(g) + 1 e^- → P_(g)^3-

2^nd Electron Affinity is the enthalpy change when 1 mole of gaseous  1- ions gains 1 mol of electrons to be converted to 1 mol of gaseous 2- ions.

Does the following equation represent reaction for 2nd Electron affinity.

N^- _(g) + 1 e^- → N_(g)^2-