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.

Select the strongest intermolecular force in each of the following. 1) Cl2 – 2) C2H6 – 3) NF3 – 4) BF3 – 5) CH3Cl –

How much heat (in J), is necessary when 54.0 g of ice at

Calculate the pH of a solution with a hydroxide ion concentration of 5.25 x 10-6 M at 25oC.

Calculate the pH of a buffer containing 2.50 M formic acid, HCOOH (Ka = 1.8 × 10-4) and 1.25 M sodium formate, HCOONa.You must show all of your work for credit.

Determine the Ka for CH3NH3+ at 25°C. The Kb for CH3NH2 is 4.4 × 10-4.

Given the following equation and equilibrium constant: 2H2(g) + S2(g)  ⇌ 2H2S(g)    K = 1.08 x 107 determine K for the following reaction H2S(g)  ⇌ H2(g)  + S2(g)  K = ?

Phosphorus pentachloride decomposes into phosphorus trichloride and chloring gas at 250oC. PCl5(g) ⇌ PCl3(g) + Cl2(g) If 0.98 M PCl5, 0.188 M PCl3 and 0.188 M Cl2 are present at equilibrium: Show all your work and setup for credit. A) Calculate KC for this reaction. B) Calculate KP for this reaction.

What is the freezing point of a solution of 9.25 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) 

The half-life of a first-order reaction is 0.300 s. What is the rate constant?