The dissolution of ammonium nitrate, NH4NO3, in water is an endothermic process. Since the calorimeter is not a perfect insulato
r, will the enthalpy of solution for ammonium nitrate be reported as too high or too low if this heat change is ignored? Explain
1 answer:
Answer:
Explanation: As already mentioned that the dissolution of ammonium nitrate in water is an endothermic process, which explains that more energy would be needed to break the bond between the reactants rather than the formation of the products.
Hence, the enthalpy of the solution for ammonium nitrate would be positive in nature as energy is being given to the reactants molecules to get converted into the products.
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Answer : The entropy change of reaction for 1.62 moles of reacts at standard condition is 217.68 J/K
Explanation :
The given balanced reaction is,
The expression used for entropy change of reaction is:
where,
= entropy change of reaction = ?
n = number of moles
= standard entropy of formation
= 245.463 J/mol.K
= 202.78 J/mol.K
= 292.53 J/mol.K
Now put all the given values in this expression, we get:
Now we have to calculate the entropy change of reaction for 1.62 moles of reacts at standard condition.
From the reaction we conclude that,
As, 2 moles of has entropy change = 268.74 J/K
So, 1.62 moles of has entropy change =
Therefore, the entropy change of reaction for 1.62 moles of reacts at standard condition is 217.68 J/K