estimate the change in energy when solid rubidium reacts with gaseous diatomic chlorine molecules. Express your answer in units of kJ/mole
delta H = Ecryst+Evaporization+E(Rb, ionization)+Edissociation+Eaffinity
What is Ecryst??
what is it?
-430.5
To estimate the change in energy when solid rubidium reacts with gaseous diatomic chlorine molecules, we can make use of the concept of the standard molar enthalpy of formation.
The standard molar enthalpy of formation (ΔHf) is the change in enthalpy (energy) when one mole of a compound is formed from its constituent elements in their standard states at a given temperature and pressure. In this case, we want to find the ΔHf for the reaction where solid rubidium (Rb) reacts with gaseous diatomic chlorine (Cl₂) to form rubidium chloride (RbCl).
To find the ΔHf for RbCl, we need to know the values of the standard molar enthalpies of formation for Rb(s) and Cl₂(g). These values can be found in reference tables or databases.
Assuming the standard molar enthalpy of formation for RbCl is -347 kJ/mol, we can write the balanced chemical equation for the reaction:
2Rb(s) + Cl₂(g) → 2RbCl(s)
Since the stoichiometric coefficient for RbCl is 2, the change in energy for the reaction can be calculated by multiplying the ΔHf value by the stoichiometric coefficient:
ΔH = 2 * ΔHf
ΔH = 2 * -347 kJ/mol
ΔH ≈ -694 kJ/mol
Therefore, the estimated change in energy when solid rubidium reacts with gaseous diatomic chlorine molecules is approximately -694 kJ/mol.