Solution Found!
Answer: At a certain temperature and a total pressure of
Chapter 14, Problem 72P(choose chapter or problem)
At a certain temperature and a total pressure of 1.2 atm, the partial pressures of an equilibrium mixture
\(2 A(g)\ \leftrightharpoons\ B(g)\)
are \(P_{A}=0.60\ \mathrm{atm}\) and \(P_{B}=0.60\ \mathrm{atm}\). (a) Calculate the \(K_{p}\) for the reaction at this temperature. (b) If the total pressure were increased to 1.5 atm, what would be the partial pressures of A and B at equilibrium?
Questions & Answers
QUESTION:
At a certain temperature and a total pressure of 1.2 atm, the partial pressures of an equilibrium mixture
\(2 A(g)\ \leftrightharpoons\ B(g)\)
are \(P_{A}=0.60\ \mathrm{atm}\) and \(P_{B}=0.60\ \mathrm{atm}\). (a) Calculate the \(K_{p}\) for the reaction at this temperature. (b) If the total pressure were increased to 1.5 atm, what would be the partial pressures of A and B at equilibrium?
ANSWER:Step 1 of 5
In this, we need to use the law of mass action to write equilibrium expression in terms of partial pressure and put the values of partial pressure of species and 
Given data
The partial pressure of species A 
The partial pressure of species B 
The total, partial pressure 