At 400 K, the Kc is equal to 2.6 x 10⁻⁵ for the reaction given below. What is the Kp of the reaction at this temperature given that R = 0.0821 L-atm/mol-K? 2NH3(g) ⇌  N2(g) + 3H2(g)

A. At 400 K, the Kc is equal to 2.6 x 10⁻⁵ for the reaction given below. What is the Kp of the reaction at this temperature given that R = 0.0821 L-atm/mol-K?

2NH_3(g) ⇌  N_2(g) + 3H_2(g)

B. In a 1.00 L flask, 0.600 mol of Br2 and 0.600 mol of Cl2 are placed and allowed to reach equilibrium in a reaction given below. After reaching equilibrium, the flask is found to contain 0.280 mol of BrCl. What is the value of Keq for this reaction?

Br_2(g) + Cl_2(g)  ⇌  2BrCl_(g)

C. At 308 K, the reaction indicated has a Keq value equal to 1.60 x 10⁻⁵. Calculate the concentration of NO at equilibrium if 3.00 mol of pure NOCl was initially placed in a 2.00 L flask.

2NOCl_(g)   ⇌  2NO_(g) + Cl_2(g)

D. A 0.50 M concentration of weak base, CH3NH2, was found to ionize at 1.7%. What is the concentration of CH3NH3⁺ in the solution?

E. A solution has a H₃O⁺ concentration of 1.3 x 10⁻⁴. What is the pOH of the solution at 25°C?

F. Consider the equilibrium reaction: YZ_3(s) ⇌ Y³⁺_(aq) + 3Z^-_(aq). What is the solubility of YZ₃ (MM =78.07 g/mol) in mg/L at 25⁰C if its Ksp is 4.0 x 10⁻¹¹?

G. The concentration of B⁻ in a saturated solution of AB₃ is 1.10 x 10⁻⁵ mg/L. What is the Ksp of AB₃ if the MM of B is 17.0 g/mol?