E. A reaction vessel contains NH3, N₂, and H₂ at equi- librium at a certain temperature. The equilibrium concentrations are [NH₂] = 0.25 M. [N₂] = 0.11 M. and [H₂] 1.91 M. Calculate the equilibrium con- stant K for the synthesis of ammonia if the reaction is represented as (a) N₂(g) + 3H₂(g) 2NH₂(g) (b) N₂(g) + H₂(g)NH₂(g)

The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.

A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer

For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?