Question

Use the data given here to calculate the values of AGfxn at 25 °C for the reaction described by the equation Compound AG; (kJ/mol) +387.7 -623.9 В A B C +402.0 С AGxn = kJ If AHixn and ASPxn are both negative values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is O enthalpy-driven to the left. entropy-driven to the left. O enthalpy-driven to the right O entropy-driven to the right

Answer 1

(1.) $\Delta$ G^o_rxn = 638.2 kJ

(2.) The spontaneous reaction is : entropy-driven to the right

Explanation

The given reaction is : A + B $\rightleftharpoons$ C

$\Delta$G^o_rxn = $\Delta$ G^o_f products - $\Delta$ G^o_f reactants

$\Delta$G^o_rxn = $\Delta$ G^o_f C - [$\Delta$G^o_f A + $\Delta$ G^o_f B]

$\Delta$G^o_rxn = (402.0 kJ/mol) - [(387.7 kJ/mol) + (-623.9 kJ/mol)]

$\Delta$G^o_rxn = 402.0 kJ - 387.7 kJ + 623.9 kJ

$\Delta$G^o_rxn = 638.2 kJ