From the following data, calculate the standard enthalpy change for the combustion of cyclopropane at 298 K: The standard enthalpy of formation of , and propene(g) are - 393.5, - 285.8 and respectively. The standard enthalpy of isomerization of cyclop

Question

From the following data, calculate the standard enthalpy change for the combustion of cyclopropane at 298 K:

The standard enthalpy of formation of ${CO}_{2} (g)$ , $H_{2} O (l)$ and propene(g) are - 393.5, - 285.8 and $20.42 kJ {mol}^{- 1}$ respectively.

The standard enthalpy of isomerization of cyclopropane to propene is $- 33.0 kJ {mol}^{- 1}$ .

Report your answer by rounding off to the nearest integer [magnitude only].

Smart Achievers · Accepted Answer

(2091)

${CO}_{2} (g)$

$Δ_{c} H_{(Propene)}^{Θ} = [3 Δ_{f} H_{({CO}_{2})}^{Θ} + 3 Δ_{f} H_{(H_{2} O)}^{Θ}] - [Δ_{f} H_{(Propene)}^{Θ} + \frac{9}{2} Δ_{f} H_{O_{2}}^{Θ}]$

$= 3 (- 393.5) + 3 (- 285.8) - (20.42) = - 2058.32 kJ {mol}^{- 1}$

$To the above reaction, if we add the reaction:$

$∴$ $Δ_{c} H_{(cyclopropane)}^{Θ} = (- 2058.32 - 33.0) kJ {mol}^{- 1} = - 2091.32 kJ {mol}^{- 1}$

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