For the reaction SbCl₅(g) $\leftrightharpoons$ SbCl₃(g) + Cl₂(g),
$\Delta$ G^$\circ$_f (SbCl₅) = -334.34 kJ/mol
$\Delta$ G^$\circ$_f (SbCl₃) = -301.25 kJ/mol
$\Delta$ H^$\circ$_f (SbCl₅) = -394.34 kJ/mol
$\Delta$ H^$\circ$_f (SbCl₃) = -313.80 kJ/mol
This reaction proceeds spontaneously at 298 K and 1 atm pressure.

Question

For the reaction SbCl₅(g)

\leftrightharpoons

SbCl₃(g) + Cl₂(g),

\Delta

G^$\circ$_f (SbCl₅) = -334.34 kJ/mol

\Delta

G^$\circ$_f (SbCl₃) = -301.25 kJ/mol

\Delta

H^$\circ$_f (SbCl₅) = -394.34 kJ/mol

\Delta

H^$\circ$_f (SbCl₃) = -313.80 kJ/mol
This reaction proceeds spontaneously at 298 K and 1 atm pressure.

Quizplus · Accepted Answer

The Answer of For the reaction SbCl₅(g) $\leftrightharpoons$ SbCl₃(g) + Cl₂(g), $\Delta$G^$\circ$_f (SbCl₅) = -334.34 kJ/mol $\Delta$G^$\circ$_f (SbCl₃) = -301.25 kJ/mol $\Delta$H^$\circ$_f (SbCl₅) = -394.34 kJ/mol $\Delta$H^$\circ$_f (SbCl₃) = -313.80 kJ/mol This reaction proceeds spontaneously at 298 K and 1 atm pressure.

For the Reaction SbCl5(g) ⇋\leftrightharpoons⇋ SbCl3(g) + Cl2(g) Δ\DeltaΔ G ∘\circ∘ f (SbCl5) = -334

For the Reaction SbCl₅(g) $\leftrightharpoons$ SbCl₃(g) + Cl₂(g) $\Delta$ G^$\circ$_f (SbCl₅) = -334