Find tge enthalpy of formation of diaonond from graphite
Answers
The enthalpy difference between graphite and diamond
The enthalpy difference between graphite and diamond is too large for both to have a standard enthalpy of formation of zero. To determine which form is zero, the more stable form of carbon is chosen. This is also the form with the lowest enthalpy, so graphite has a standard enthalpy of formation equal to zero.
some important points
The standard enthalpy of formation is a measure of the energy released or consumed when one mole of a substance is created under standard conditions from its pure elements. The symbol of the standard enthalpy of formation is ΔHf.
Δ = A change in enthalpy
o = A degree signifies that it's a standard enthalpy change.
f = The f indicates that the substance is formed from its elements
The equation for the standard enthalpy change of formation (originating from Enthalpy's being a State Function), shown below, is commonly used:
ΔHoreaction=∑ΔHof(products)−∑ΔHof(Reactants)(3.6.1)
This equation essentially states that the standard enthalpy change of formation is equal to the sum of the standard enthalpies of formation of the products minus the sum of the standard enthalpies of formation of the reactants.