Equilibrium Constant (Kc or Keq)

If the equilibrium constant is much greater than one (K >> 1) then

• Equilibrium is not established.
• Equilibrium lies to the right (products are favored)
• Equilibrium lies to the left (reactants are favored)
• Neither products or reactants are favored.

If the equilibrium constant is much less than one (K << 1) then

• Equilibrium is not established.
• Equilibrium lies to the right (products are favored)
• Equilibrium lies to the left (reactants are favored)
• Neither products or reactants are favored.

In the equation K_c = K_p(RT)^Δn , the Δn means

• The sum of all the moles.
• moles of products - moles of reactants
• moles of reactants - moles of product
• reaction order

N₂O₄(g) ↔ 2 NO₂(g)
What is the concentration equilibrium constant expression?

• K_c = [NO₂]²/[N₂O₄]
• K_c = [N₂O₄]/[NO₂]²
• K_c = [N₂O₄]²/[NO₂]
• K_c = [NO₂]/[N₂O₄]²

Tags

NGSS.HS-PS1-7

N₂O₄(g) ↔ 2 NO₂(g)
What is the equilibrium constant expression?

• K_p = (P_NO2)²/ (P_N2O4)
• K_p = (P_N2O4) / (P_NO2)^₂
• K_p = (P_N2O4)² / (P_NO2)
• K_p = (P_NO2) / (P_N2O4)²

For the equilibrium
2SO₃(g) ↔ 2SO₂(g) + O₂(g)
K_c = 4.08x10^-3 at 1000K
What is K_p?

• 3.45 x 10⁵
• 2.99
• 0.335
• 3.4 x 10^-5

What is the equilibrium-constant expression for 
CO₂(g) + H₂(g) ↔ CO(g) + H₂O(l)

• K_c= [CO][H₂O] / [CO₂][H₂]  
• K_c= [CO₂][H₂] / [CO]
• K_c= [CO₂][H₂] / [CO][H₂O]
• K_c= [CO] / [CO₂][H₂]  

Find the K_c for
2NOBr(g) + Cl₂(g) ↔ 2NO(g) + 2BrCl(g)
 if 
2NOBr(g) ↔ 2NO(g) + Br₂(g)
has a K_c = 0.014
Br2(g) + Cl2(g) ↔ 2BrCl(g)
has a K_c = 7.2

• 0.10
• 10
• 1.0 x 10^-3
• 1.0 x 10^-2