Honors Chemistry                                                                        Name_____________________________

Equilibrium constants PMP

Mr. McAfoos                                                                                 Period_______ Date__________________

 

Write the formula for K for each of the following UNBALANCED reactions:

  1. H2 + Cl2 ⇄ HCl
  2. Ba(NO3)2 + Al2(SO4)3 ⇄ Al(NO3)3 + BaSO4
  3. C12H22O11 + O2 ⇄ CO2 + H2O
  4. NO2 ⇄ N2O4
  5. Fe+3 + SCN-1⇄ FeSCN+2 (don’t worry about charges when you balance …formulas are correct)
  6. 2A + Q + R ⇄ 3B
  7. 4B ⇄ T + Z +2Q

 

  1. The reaction 3R + T ⇄ 2B + A is at equilibrium when the [R] = 4.2M, [T] = 3.3M, [B] = 0.00442M and [A] = 1.000M. What is the value of K?

 

  1. If the reaction in #8 is at equilibrium and the [R]=1.76M, [T]=2.222M, and [A]=2.31M, what is the concentration of B?

 

  1. At equilibrium the [NO2] = 2x10-4 M while the [N2O4] = 2.11 M.  What is the value of K?

 

  1. If the reaction above is at equilibrium and the [N2O4] = 1.55 M, what is the concentration of the NO2?

 

  1. For each of the following cases, determine whether or not the mixture is at equilibrium and if it is not determine what direction the reaction will shift to reach equilibrium.

a) [N2O4] = 4.00, [NO2] = 8.7x10-3

b) [N2O4] = [NO2] = 3.11 M

c) [N2O4] = 3.1x10-4 M, [NO2] = 2.44 M

d) [N2O4] = 0.335 M, [NO2] = 7.97 x10-5 M

e) [N2O4] = 0.00 M, [NO2] = 1.20 M

f) [N2O4] = 4.55 M, [NO2] = 0.00 M