enthalpy H i the sum of the internal energy U and the 'pV-energy'= p*V.
The pV term is also called flow-energy, pressure-energy or energy of displacement. The p is the external pressure, but for systems at constant pressure it is also equal to the internal pressure. Hence: H=U+pV.
It follows that H is a composite form of energy, a statement not commonly found in the literature.
>> 'Energy-balance of the Joule-Thomson experiment: Enthalpy change at decompression.' (NPT-procestechnologie, 2010, 17(4)18-22)
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A negative enthalpy of formation indicates that energy is evolved.
The 1st step would be to give an example of the equation to be solved.
I think you're going to have to give us the equation first, dear
If you have two equations give AND one parametric equation why do you need to find yet another equation?
To solve Hess's law problems, first write out the chemical equations for all reactions involved. Then calculate the enthalpy change for each reaction. Finally, add or subtract the enthalpy changes to obtain the overall enthalpy change for the desired reaction.
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
The difference between the enthalpy of formation of the products minus the enthalpy of formation of the reactants is the enthalpy of the reaction
CH3CHO+HCl
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"Try as he might, he could not solve the equation."
The enthalpy change to burn 37.5 g of ammonia (NH3) can be calculated using the standard enthalpy of formation of ammonia and the balanced chemical equation for its combustion. The enthalpy change will depend on the specific conditions of the reaction, such as temperature and pressure.
NaCl+H2O COMPELATE THE EQUATION
Heat appears in the equation as either a reactant (if heat is added to the reaction) or as a product (if heat is released by the reaction). It is typically denoted by the symbol "ΔH" for the change in enthalpy.
Specific Heat is:-the amount of energy required to raise the temperature of 1g of a substance 1°C-specific heat is symbolised as Cp or C-has units of J/g °C-J stands for Joules, which is a unit of energyMost often used in equation: q = mΔTCpq = energy in Jm = mass in gΔT = change in temperatureCp = specific heatExampleHow much energy is required to raise the temperature of 345.34g of Aluminium from 35.0°C to 250.00°C ? The specific heat of Aluminium is .90 J/Cp q = mΔTCpq = 345.34g(250.00°C - 35.0°C)0.09J/g°Cfrom there its just simple Algebra.q = 66,823.29JHowever, not all problems will be as simple as the one above. Some may require up to 3+ equations that can include Enthalpy or ΔH which leads to using a Change of State Graph.
A thermochemical equation includes the enthalpy change of a reaction, whereas a traditional chemical equation only shows the reactants and products involved in a reaction without considering energy changes. Thermochemical equations provide information about the heat absorbed or released during a reaction, while traditional chemical equations focus on the chemical identities of the species involved.