Question

Part A -

At 100^oC, The equilibrium constant for the reaction:

CF₄(g) + 2H₂O(g) ⇌CO₂(g) + 4HF(g)    is   K_c,1 = 5.9

And the equilibrium constant at 100^oC for the reaction:

CO(g) + ½ O₂(g) ⇌ CO₂(g)                      is   K_c,2 = 1.3

Compute the equilibrium constant at 100^oC for the reaction (2 sig figs)

2 CF₄(g) + 4H₂O(g) ⇌2CO(g) + 8HF(g) + O₂(g)          is K_c,3 = ?

Part B -

Consider the reaction below (Equilibrium Constant @ 300K = K_p = 0.150)

A₂B₂(g) + 2B₂(g) ⇌ A₂B₆(g).   

If 0.500 atm of A₂B₂, 0.500 atm of B₂ and 1.00 atm of A₂B₆ are combined and allowed to react, the total pressure at equilibrium is ______ atm. (3 sig figs). Enter numerical answer only.

Part C -

Consider the decomposition of solid ammonium carbonate at 25° C:

(NH₄)₂CO₃(s) ⇌CO₂(g) + 2 NH₃(g) + H₂O(l)       Kp = 7.80

The partial pressure of NH₃ at equilibrium is _______ atm. (enter numerical answer only)

Part D -

An equilibrium mixture of A₂, B₂ and AB at 458^oC contains 0.112 atm A₂, 0.112 atm B₂ and 0.775 atm AB. The equilibrium pressure of A₂(g) after 0.100 atm of AB is added into the vessel and the equilibrium is reestablished is _________ atm. (3 sig figs) 2 AB(g)   ⇌ A₂(g) + B₂(g)

Part E -

The equilibrium below begins with only pure SO₃(g) in a 2.50-L flask at 300^oC. At equilibrium the mass of SO₃(g) remaining is 2.21 grams.                           

2SO₃(g) ⇌2SO₂(g) + O₂(g)            K_c=0.345

The concentration of SO₂ at equilibrium is ________ M. (enter numerical answer only)

Answer 1