For the reaction below, Kp= 28.63 at 800 K. Calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PpCl5=0.5600 atm and PpCl3= 0.4700 atm

PCl5(g) <--> PCl3(g) + Cl2(g)

PCl5=??
PCl3=??
Cl2=??

1 answer

42
Similar Questions
  1. At 930 K, Kp = 0.30 for the following reaction.2 SO2(g) + O2(g)=>2 SO3(g) Calculate the equilibrium partial pressures of SO2,
    1. answers icon 1 answer
  2. 3H2(g)+N2(g)=2NH3(g)Suppose the equilibrium constant Kp = 0.003337 for the reaction above. If the equilibrium mixture contains
    1. answers icon 1 answer
    1. answers icon 1 answer
  3. given the equilibrium constant for the following reaction at 500 K,2 NO (g) + O2 (g) <==> 2 NO2 (g) Kc = 6.2x10^5 calculate the
    1. answers icon 2 answers
more similar questions