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-PS1-6

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-PS1-6

This symbol indicates that a reaction is ____________

• reversible
• irreversible

Tags

NGSS.HS-PS1-6

Which is the reactant - and why?

• A, as concentration decreases
• B, as concentration decreases
• A, as concentration increases
• B, as concentration increases

Tags

NGSS.HS-PS1-5

At what time the reaction reached equilibrium?

• t₁
• t₂
• t₃
• t₄

Tags

NGSS.HS-PS1-6

When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in

• Chemical Equilibrium
• Chemical Balance
• Stoichiometry
• Chemical Reaction

Tags

NGSS.HS-PS1-6

The following factors affect the position of equilibrium EXCEPT

• Concentration
• Pressure
• Temperature
• States of matter

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

2SO_2(g)+O_2(g) ⇌ 2SO_3(g) + Heat

Adding SO_2(g) will

• shift equilibrium right

• shift equilibrium left

• increase rate of reaction

• have no change

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

2SO₂(g)+O₂(g) ⇌ 2SO₃(g) + Heat

Increasing the temperature will...

• shift equilibrium right

• shift equilibrium left

• increase pressure

• have no change

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

2SO_2(g) + O_2(g) ⇌ 2SO_3(g) + Heat

Removing O_2(g) will

• shift equilibrium right

• shift equilibrium left

• increase pressure

• have no change

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6