The problem of calculating the reaction heat of compounds
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This post was last edited by tcs1789@163.com on 2010-8-30 16:39. The standard enthalpy of formation for (NH4)2SO4 is -280.66 kcal/mol, that for NH3 is -11.02 kcal/mol, and that for H2SO4 is -217.32 kcal/mol. How can we calculate the enthalpy of formation for the reaction between sulfuric acid and ammonia?
Write the standard thermochemical equation and balance it, making sure that the phases correspond correctly. The reaction enthalpy is the sum of the enthalpies of each substance, with the coefficients serving as the weights.
Go and check out some books on physical chemistry; they should explain these things. I forgot, haha!
Hehe. . . . Well, it’s a question from a physical chemistry book!
I feel like the conditions given aren’t sufficient; it should be impossible to do the calculation based on just these conditions.
First, find the standard enthalpy values of the reactants and products, then subtract the total enthalpy of the reactants from the total enthalpy of the products. A negative value indicates heat release, while a positive value indicates heat absorption. The prerequisite is to balance the chemical equation
The sixth floor is the correct answer, but it’s essential to clarify the state of the substance under the reaction conditions.
“How can the enthalpy of formation for the reaction between sulfuric acid and ammonia be calculated? ”? There seems to be a problem with this sentence. Enthalpy of formation refers to that of the substance, not to that of the reaction. For chemical reactions, it is either the heat of reaction or the heat of combustion. It probably refers to the heat of reaction here.
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