A diagram showing the application of Hess' law to reaction enthalpy calculated from enthalpies of formation.
Apply Hess's law to calculate standard enthalpy of reaction from standard enthalpies of formation.
What is the difference between the outputs of the following two queries?
Sum up the enthalpies of formation of the reaction products.
The mechanism of solid-state transformation is similar.
This curve can be used to calculate enthalpies of transitions.
Add up the enthalpies of formation of the reagents of the reaction.
The enthalpy change of a reaction is equal to the sum of the enthalpies of formation of the products minus the sum of the enthalpies of formation of the reactants.
use the following standard enthalpies of combustion at 298 K (given in kJ mol-1)
therefore, the Standard Enthalpy of formation for H2O(l) is
In a general way, the enthalpy of a reaction is the sum of the enthalpies of formation of the products minus the enthalpies of formation of the reactants, each one multiplied by its stoichiometric coefficients.
In this case, we know the enthalpies of formation for the following reactions:[3]
It is the sum of enthalpy of the various states, liquid (water) and gas (vapour).
It is the sum of enthalpy of the various states, liquid (water) and gas (vapour).
The next bar chart shows the lattice enthalpies of the Group 1 chlorides.
Requêtes fréquentes français :1-200, -1k, -2k, -3k, -4k, -5k, -7k, -10k, -20k, -40k, -100k, -200k, -500k, -1000k,
Requêtes fréquentes anglais :1-200, -1k, -2k, -3k, -4k, -5k, -7k, -10k, -20k, -40k, -100k, -200k, -500k, -1000k,
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