7.2 Kc and Qc

K_c for the reaction can be written as

• K_c = [NO₂]²/[N₂O₄]¹
• K_c = [N₂O₄]¹/[NO₂]²
• K_c = [NO₂]/[N₂O₄]
• K_c = [N₂O₄]/[NO₂]

K_c^' is written as

• K_c^' = 2K_c
• K_c^' = 1/K_c
• K_c^' = K_c²
• K_c^' = K_c

K_c^' is written as

• K_c^' = 2K_c
• K_c^' = 1/K_c
• K_c^' = K_c²
• K_c^' = K_c

K_c^' is written as

• K_c^' = ½K_c
• K_c^' = 1/K_c
• K_c^' = K_c^½
• K_c^' = K_c²

Calculate K_c^' if K_c = 200

• K_c^' = 100
• K_c^' = 20
• K_c^' = √200
• K_c^' = √100

Which of the following is FALSE about Q_c and K_c?

• Qc reaction quotient at a particular time and varies over time
• K_c is equilibrium constant, which is fix at a fixed temp
• Q_c will eventually equal to K_c over time
• Q_c does not change

What will happen when Q_c is less < than K_c?

• Equilibrium is disturbed
• Equilibrium contain more products than reactants
• Equilibrium will shift to the right to increase Q_c
• Equilibrium will shift to the left to decrease Q_c

Tags

NGSS.HS-PS1-6

What will happen when Q_c is greater > than K_c?

• Equilibrium is disturbed
• Equilibrium contain more reactants than products
• Equilibrium will shift to the right to increase Q_c
• Equilibrium will shift to the left to decrease Q_c

Tags

NGSS.HS-PS1-6