for the reaction N₂O₅(s)$\rightarrow$ 2NO₂(g)+ ½O₂(g),$\Delta$H_r = 109.5 kJ.mol^-1 at 298 K at constant temperature and pressure,$\Delta$H $\Delta$U.

Question

for the reaction N₂O₅(s)$\rightarrow$ 2NO₂(g)+ ½O₂(g),$\Delta$H_r = 109.5 kJ.mol^-1 at 298 K at constant temperature and pressure,$\Delta$H > $\Delta$U.

Quizplus · Accepted Answer

Since the enthalpy change is positive and the reaction is at constant temperature and pressure, the internal energy change must also be positive. Therefore, ΔH > ΔU and statement A is true.

For the Reaction N2O5(s) →\rightarrow→ 2NO2(g)+ ½O2(g) Δ\DeltaΔ Hr = 109 Δ\DeltaΔ H >

For the Reaction
N₂O₅(s) $\rightarrow$ 2NO₂(g)+ ½O₂(g) $\Delta$ H_r = 109 $\Delta$ H >