Given the ∆H°_f, calculate the ∆H°_rxn for the formation of diamond from graphite. ∆H°_f C, graphite) = 0 kJ/mol
∆H°_f C, diamond) = 2 kJ/mol

Question

Given the ∆H°_f, calculate the ∆H°_rxn for the formation of diamond from graphite. ∆H°_f C, graphite) = 0 kJ/mol ∆H°_f C, diamond) = 2 kJ/mol

Quizplus · Accepted Answer

The formation of diamond from graphite can be considered as a reaction where graphite is converted into diamond. Given that the enthalpy of formation (∆H°f) for graphite is 0 kJ/mol and for diamond is 2 kJ/mol, the reaction enthalpy (∆H°rxn) is simply the difference in the enthalpy of formation of the products and reactants. Since graphite is the reactant and its ∆H°f is 0, and diamond is the product with a ∆H°f of 2 kJ/mol, the ∆H°rxn for the formation of diamond from graphite is +2 kJ/mol.

Given the ∆H°f, Calculate the ∆H°rxn for the Formation of Diamond

Given the ∆H°_f, Calculate the ∆H°_rxn for the Formation of Diamond