Asked by MIndy
Phosphorus trichloride gas and chlorine gas reacts to form phosphorus pentachloride gas: PCL3(g) +CL2(g) = PCL5(g). A vessel is CHARGED WITH A MIXTURE OF PCL3(g) and CL2(g), which is allowed to equilibrate at 450K. At equlibrium the partial pressures of the three gases are Ppcl3=0.124atm, Pcl2 = 0.157 atm, and Ppcl5 = 1.30 atm. (a) what is the value of Keq at this temperature? Does the equilibrium favor reactants or products?
Answers
Answered by
DrBob222
If you want Kp is it
Kp = (PCl5)/(PCl3)(Cl2)
Substitute and solve for Kp.
I assume Keq is Kc although I don't know that. You can convert Kp to Kc by
Kp = Kc(RT)<sup>delta n</sup)
where delta n = #n products- #n reactants = 1-2 = -1
Kp = (PCl5)/(PCl3)(Cl2)
Substitute and solve for Kp.
I assume Keq is Kc although I don't know that. You can convert Kp to Kc by
Kp = Kc(RT)<sup>delta n</sup)
where delta n = #n products- #n reactants = 1-2 = -1
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.