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

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
Calculate the value of the equilibrium constant (K_p) at 800 K and 1 atm pressure.

A) 1.31 * 10³
B) 1.11 * 10³
C) 1.91 * 10²
D) 1.71 * 10²
E) None of the above