Equilibrium constant calculations

The equilibrium constants for the following two reactions are:

                                                            A ⇌ 2 D + C                           K = 1.55

                                                            2 B ⇌ 2 D                               K = 50.2

What must e the value of K for the following overall reaction?        A ⇌ 2 B + C

• 32.4

• 0.000397

• 2.44 × 10^-3

• 0.0309

• 0.0199

A closed vessel was filled with the two reactants, each at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of BrCl(g)?

    Br₂(g) + Cl₂(g) ⇌ 2 BrCl(g)               K_p = 1.2 × 10^-5

• 0.0041 atm

• 0.023 atm

• 0.0034 atm

• 0.029 atm

• 0.0017 atm

• 594

• 7070

• 116

• 41.0

• 5120

Assume the reaction below is initially at equilibrium. Which direction (forward or backward) does equilibrium shift to upon each of the following changes?                                                                                                                                                                                           

                                                N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)               ∆H˚ = - 91.8 kJ/mol

 

A)    Increased N₂ gas__

 

B)    Increased H₂ gas__

 

C)    removed NH₃ gas__

 

D)    removed H₂ gas__

 

E)     raised the temperature__

 

F)     decreased the pressure__

 

G)    added an inert gas__

 

H)    increased the pressure__