In the reaction P₄(g) 2P₂(g)K_p = 0.500 atm at 1052°C. In an experiment, P₄(g) is initially placed into a container at 1052°C. The total pressure of the equilibrium mixture of P₄(g) and P₂(g) is 6.00 atm. Calculate the equilibrium pressures of P₄(g) and P₂(g). Calculate the fraction (by moles) of P₄(g) that has dissociated to reach equilibrium.

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The Answer of In the reaction P₄(g) 2P₂(g)K_p = 0.500 atm at 1052°C. In an experiment, P₄(g) is initially placed into a container at 1052°C. The total pressure of the equilibrium mixture of P₄(g) and P₂(g) is 6.00 atm. Calculate the equilibrium pressures of P₄(g) and P₂(g). Calculate the fraction (by moles) of P₄(g) that has dissociated to reach equilibrium.

In the Reaction P4(g) 2P2(g)Kp = 0.500 Atm at 1052°C

In the Reaction P₄(g) 2P₂(g)K_p = 0.500 Atm at 1052°C