A. Co + H₂O ⇄ co₂+ H₂
= -8.314[tex]\frac{J}{K.mol}[/tex] x298k x In (6.54x16³)
= -21.77 kJ/m0/
for 2.32 molco, A = -21.77×2-32
= -50.51kj/mol
B. Fe₂03(5) +3H₂(9) ⇄ 2 Fe(s) + 3H₂0(9)
= -8.314 × 298x/n (2.47x10⁻¹⁰)
= +54.807 kJ/mol
for 1.61 mol fe₂03, Δ4= 54.807 X 1.61 mol
= 88.24 kJ/mol.
Equilibrium constant numbers are obtained by allowing a single reaction to reach equilibrium and measuring the concentrations of each substance involved in the reaction. The ratio of product concentration to educt concentration is calculated. A mathematical ratio indicating product concentration divided by reactant concentration.
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