We need to know the change in enthalpy for dry ice sublimation.
Change in enthalpy for dry ice sublimation is: + 427.4 KJ/mol
The enthalpy of dry ice sublimation is the energy required to melt one mole of dry ice into liquid.
Enthalpy of formation is opposite of enthalpy of sublimation.
Given, enthalpies of formation is -427.4 KJ/mol, so, enthalpy of sublimation= +427.4 KJ/mol.
The change in enthalpy for dry ice sublimation is 33.9 kJ.
Let's consider the equation for the sublimation of dry ice.
CO₂(s) ⇄ CO₂(g)
Given the standard enthalpies of formation (ΔH°f), we can calculate the standard enthalpy change of sublimation (ΔH°s) using the following expression.
[tex]\Delta H\°_s = \Sigma \Delta H\°_f(p) \times n_p - \Sigma \Delta H\°_f(r) \times n_r[/tex]
where,
[tex]\Delta H\°_s = \Delta H\°_f(CO_2(g)) \times 1mol - \Delta H\°_f(CO_2(s)) \times 1mol\\\\\Delta H\°_s = (-393.5kJ/mol) \times 1mol - (-427.4 kJ/mol) \times 1mol = 33.9kJ[/tex]
The change in enthalpy for dry ice sublimation is 33.9 kJ.
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