Consider the reaction between and at K. Under standard conditions, each species has a partial pressure of 1 atm. If a flask contains 0.500 atm of and 0.500 atm of , calculate the partial pressure of hydrogen at equilibrium.
Liquid is dark blue at low temperatures, but the color fades and becomes greenish at higher temperatures as the compound decomposes to and . At 25℃, a value of = 1.91 has been established for this decomposition. If 0.236 moles of are placed in a 1.52-L vessel at 25℃, what is the equilibrium partial pressure of ?
Nitrogen oxides are air pollutants produced by the reaction of nitrogen and oxygen at high temperatures. At ℃, the value of the equilibrium constant for the reaction, , is . Calculate the equilibrium concentration of in air at ℃ if = 0.036 M and = 0.0089 M when equilibrium is reached.