rom these data,→+Srhombic O2g SO2g =ΔH°rxn−296.06kJmol→+Smonoclinic O2g SO2g =ΔH°rxn−296.36kJmolCalculate the enthalpy change for the transformation:→Srhombic Smonoclinic(Monoclinic and rhombic are different allotropic forms of elemental sulfur.)Be sure your answer has the correct number of significant digits.kJmol
Question
rom these data,→+Srhombic O2g SO2g =ΔH°rxn−296.06kJmol→+Smonoclinic O2g SO2g =ΔH°rxn−296.36kJmolCalculate the enthalpy change for the transformation:→Srhombic Smonoclinic(Monoclinic and rhombic are different allotropic forms of elemental sulfur.)Be sure your answer has the correct number of significant digits.kJmol
Solution
The enthalpy change for the transformation from rhombic sulfur to monoclinic sulfur can be calculated using Hess's Law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for each step in the reaction.
Here, we have two reactions:
- Rhombic S + O2 -> SO2, ΔH°rxn = -296.06 kJ/mol
- Monoclinic S + O2 -> SO2, ΔH°rxn = -296.36 kJ/mol
We want to find the enthalpy change for the transformation:
- Rhombic S -> Monoclinic S
We can rearrange the first two reactions to get:
- SO2 -> Rhombic S + O2, ΔH°rxn = 296.06 kJ/mol
- Monoclinic S + O2 -> SO2, ΔH°rxn = -296.36 kJ/mol
Adding these two reactions together gives us the desired reaction:
- Rhombic S -> Monoclinic S, ΔH°rxn = -296.36 kJ/mol + 296.06 kJ/mol = -0.30 kJ/mol
So, the enthalpy change for the transformation from rhombic sulfur to monoclinic sulfur is -0.30 kJ/mol.
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