What is the standard enthalpy of formation of liquid diethylamine,(CH₃CH₂) ₂NH?
N₂O₅(g) + 8CH₄(g) → 2(CH₃CH₂) ₂NH(l) + 5H₂O(l) ; ΔH° = -1103 kJ
Substance
ΔH°_f (kJ/mol)
N₂O₅(g)
+11) 3
CH₄(g)
-74) 9
H₂O(l)
-285.8

Question

Quizplus · Accepted Answer

The standard enthalpy of formation ($\Delta H_f^\circ$) of liquid diethylamine can be calculated using the given reaction and the $\Delta H_f^\circ$ values of the reactants and products. The equation for calculating the $\Delta H_f^\circ$ of the reaction product (diethylamine) is derived from the general formula for reaction enthalpy: $\Delta H^\circ_{reaction} = \sum \Delta H_f^\circ (products) - \sum \Delta H_f^\circ (reactants)$. Rearranging this formula to solve for the $\Delta H_f^\circ$ of diethylamine gives us the correct answer.

What Is the Standard Enthalpy of Formation of Liquid Diethylamine,(CH3CH2)2NH

What Is the Standard Enthalpy of Formation of Liquid Diethylamine,(CH₃CH₂)₂NH