need help figuring this out thanks.
Show transcribed image text The equilibrium constant for the decomposition of PCl5 at 250 degree C is 0.041. PCl5(g) PCl3(g) + Cl2(g) delta H is positive; reactents and products are gases at 250 degree C. Refer to your textbook Is the reaction above exothemic or endothermic? exo What happens to the concentrations of PCl5 and Cl2 if more PCl3 is added once the reaction reaches equilibrium? (increases, decreases) PCl5 decrease Cl2 increase What happens to the moles of PCl3, PCl4 and Cl2 in the container when the pressure at which the reaction in run is increased by decreasing the volume? PCl5 PCl3 Cl2 What happens to the concentrations of PCl5, PCl3 and Cl2 when the temperature at which the reaction is run is Increased? PCl5 PCl3 Cl2 What happens to the concentrations of PCl3 and Cl2 if PCl3 is removed once the reaction reaches equilibrium? PCl3 Cl2 Does the value of the equilibrium constant, K. change in any above situations (2-5)? If so, which one(s)? Does it increase or decreases?
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