A non-equilibrium mixture of 1.00 mol of A(g) (partial pressure 1.00 atm) and 1.00 mol of B(g) (partial pressure 1.00 atm) is allowed to equilibrate at 25°C.
Calculate the partial pressure of B(g) at equilibrium.
We previously calculated the change, x, in partial pressure to achieve equilibirum, with G = 2276 J/mol and k=0.399.
We found that x=0.42959
Since the rxn moves from B to A to reach equilibrium, we lose some B while forming A. To calculate the partial pressure of B at equilibium....
PB - x = 1.00 atm - 0.42959 atm
= 0.570 atm
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