A certain chemical reaction sets up an equilibrium as follows:
A₂(g) + 3B₂(g) $\leftrightarrows$ 2AB₃(g)
At a certain temperature equilibrium is established with equilibrium partial pressures for A₂, B₂, and AB₃ of 0.11, 0.34, and 1.33 atm respectively. What is the value of the equilibrium constant at this temperature?

Question

A certain chemical reaction sets up an equilibrium as follows:
A₂(g) + 3B₂(g)

\leftrightarrows

2AB₃(g)
At a certain temperature equilibrium is established with equilibrium partial pressures for A₂, B₂, and AB₃ of 0.11, 0.34, and 1.33 atm respectively. What is the value of the equilibrium constant at this temperature?

Quizplus · Accepted Answer

The equilibrium constant $ K_p $ is calculated using the expression $ K_p = \frac{(P_{AB_3})^2}{(P_{A_2})(P_{B_2})^3} $. Substituting the given pressures: $ K_p = \frac{(1.33)^2}{(0.11)(0.34)^3} = 410 $.

A Certain Chemical Reaction Sets Up an Equilibrium as Follows ⇆\leftrightarrows ⇆

A Certain Chemical Reaction Sets Up an Equilibrium as Follows $\leftrightarrows$