Question

(1).

The equilibrium constant, K_p, for the following reaction is 1.80×10^-2 at 698K.

2HI(g) =H₂(g) + I₂(g)

If an equilibrium mixture of the three gases in a 15.5 L container at 698K contains HI at a pressure of 0.399 atm and H₂ at a pressure of 0.562 atm, the equilibrium partial pressure of I₂ is  atm.

(2).
Consider the following reaction:

PCl₅(g) =PCl₃(g) + Cl₂(g)

If 1.17×10^-3 moles of PCl₅, 0.217 moles of PCl₃, and 0.351 moles of Cl₂ are at equilibrium in a 14.9 L container at 709 K, the value of the equilibrium constant, K_p, is .

(3). The equilibrium constant, K_p , for the following reaction is 0.215 at 673 K.  

NH₄I(s) =NH₃(g) + HI(g)

If an equilibrium mixture of the three compounds in a 5.88 L container at 673 K contains 2.44 mol of NH₄I(s) and 0.217 mol of NH₃(g), the partial pressure of HI(g) is  atm.