Consider the following reaction: N2O4(g) ⇌ 2NO2(g)   Kp = 47.9 at 400 K Suppose that 2.50 atm of N2O4 decomposes and reaches equilibrium at 400 K. Determine the partial pressure of NO2 at equilibrium. Show all of your work including the ICE chart for credit.

What is the freezing point of a solution of 4.25 g of I2 (253.80 g/mol) in 50.0 g of benzene? (Freezing point of benzene = 5.5 oC, Kf for benzene = 5.12 oC/m) 

Select the strongest intermolecular force in each of the following. 1) I2 – [a] 2) CH4 – [b] 3) NF3 – [c] 4) BF3 – [d] 5) CH3Cl – [e]

A reaction vessel is charged with HI, which partially decomposes to molecular hydrogen and iodine. 2HI(g) ⇌ H2(g) + I2(g) When the system comes to equilibrium at 425oC,  partial pressure of HI = 0.708 atm, partial pressure of H2 = 0.0960 atm and partial pressure of I2 = 0.0960 atm. Show all your work and setup for credit. A) Calculate KP for this reaction. B) Calculate KC for this reaction.

Oxygen and fluorine react to form OF2. O2(g) + F2(g) ⇌ OF2(g) K = 40 at 298 K Given the information above, calculate the equilibrium constant for the following reaction at 298 K O2(g) + 2F2(g) ⇌ 2OF2(g)  K = ?

Consider the following reaction: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) If the initial concentration of Cl2 was 0.780 M and the concentration of Cl2 was 0.480 M after 166.0 s, what is the rate of the reaction?

Predict the ideal van’t Hoff factor (i) for KNO4.

For a given substance, which of the following phase transition is not endothermic?

An equilibrium that strongly favors products has ____________

Select the strongest intermolecular force in each of the following. 1) Br2 – [a] 2) CH4 – [b] 3) NH3 – [c] 4) BF3 – [d] 5) CH3Cl – [e]