At T = 250 °C the reaction PCI5(g) =PC13(g) + Cl₂(g) has an equilibrium constant in terms of pressures Kp = 2.15. (a) Suppose the initial partial pressure of PCI5 is 0.377 atm, and Ppcl3 = Pcl₂ = 0.975 atm. Calculate the reaction quotient Qp and state whether the reaction proceeds to the right or to the left as equilibrium is approached. (b) Calculate the partial pressures at equilibrium. Qp = Reaction proceeds to the PPCI5 = PPCl3 = PC1₂ atm atm atm (c) If the volume of the system is then increased, will there be net formation or net dissociation of PCI5? There will be not

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At T = 250 °C the reaction
PCI 5(g) ⇒PC13(g) + Cl₂(g)
has an equilibrium constant in terms of pressures Kp = 2.15.
(a) Suppose the initial partial pressure of PCI5 is 0.377 atm, and Ppcl3 = Pcl₂ = 0.975 atm. Calculate the reaction quotient Qp and state whether the reaction proceeds to the
right or to the left as equilibrium is approached.
(b) Calculate the partial pressures at equilibrium.
Qp =
Reaction proceeds to the
PPC15
PpCl3
PC1₂
=
II
=
atm
atm
atm
(c) If the volume of the system is then increased, will there be net formation or net dissociation of PCI5?
There will be net
Transcribed Image Text:At T = 250 °C the reaction PCI 5(g) ⇒PC13(g) + Cl₂(g) has an equilibrium constant in terms of pressures Kp = 2.15. (a) Suppose the initial partial pressure of PCI5 is 0.377 atm, and Ppcl3 = Pcl₂ = 0.975 atm. Calculate the reaction quotient Qp and state whether the reaction proceeds to the right or to the left as equilibrium is approached. (b) Calculate the partial pressures at equilibrium. Qp = Reaction proceeds to the PPC15 PpCl3 PC1₂ = II = atm atm atm (c) If the volume of the system is then increased, will there be net formation or net dissociation of PCI5? There will be net
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