Equilibrium

2SO₂(g)+O₂(g)⇌2SO₃(g)
Removing O₂(g) will

• shift equilibrium right
• shift equilibrium left
• increase pressure
• have no change

2SO₂(g)+O₂(g)⇌2SO₃(g)
Adding O₂(g) will

• shift equilibrium right
• shift equilibrium left
• decrease pressure
• have no change

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.

Tags

NGSS.HS-PS1-4

NGSS.HS-PS1-6

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.

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

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]  

Tags

NGSS.HS-PS1-7

What is the equilibrium expression for:
Fe₃O₄(s) + 4H₂(g) <--> 3Fe(s) + 4H₂O(g)

• ([Fe]³[H₂O]⁴ ) / ([Fe₃O₄][H₂]⁴)
• ([Fe₃O₄][H₂]⁴)/ ([Fe]³[H₂O]⁴)
• [H₂O]⁴ / [H₂]⁴
• ([Fe][H₂O]) / ([Fe₃O₄][H₂])

Tags

NGSS.HS-PS1-6

NGSS.HS-PS1-7

CH₄ + 2 O₂ ↔ CO₂ + 2 H₂O + 30 kJ
If CH₄ was removed, what happens to the [O₂]

• Increase
• Decrease
• Left
• Right

Tags

NGSS.HS-PS1-5

Define chemical equilibrium.

• A reaction is reversible.
• The concentration of the reactants is equal to the concentration of the products.
• The rate of a forward reaction is equal to the rate of the reverse reaction.
• The reaction stops and no further change in concentration occurs.

Tags

NGSS.HS-PS1-6

Changes in pressure will only affect substances that are in the __________ state.

• gaseous
• liquid
• solid