Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 1 atm of NOBr is sealed in a flask. At equilibrium, the partial pressure of NOBr is 0.82atm.  What is the equilibrium constant, Kp, for the reaction?

The equilibrium constant, Kp , for the following reaction is 0.215 at 673 K.NH4I(s) NH3(g) + HI(g)If an equilibrium mixture of the three compounds in a 7.23 L container at 673 K contains 2.70 mol of NH4I(s) and 0.128 mol of NH3(g), the partial pressure of HI(g) is  atm.

Consider the equilibrium between SO₂Cl₂, SO₂ and Cl₂. SO₂Cl₂(g) SO₂(g) + Cl₂(g) K 0.193 at 390 K The reaction is allowed to reach equilibrium in a 5.80-L flask. At equilibrium, [SO₂Cl₂] = 0.290 M, [SO₂] = 0.237 M and [Cl₂] = 0.237 M. (a) The equilibrium mixture is transferred to a 11.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 11.6-L flask. [SO₂Cl₂] = [SO₂] [Cl₂] = M

A chemist places 1.00 mol of each hydrogen and carbon dioxide in a 1.25-L container at 800oC. This reaction occurs:H2(g) + CO2(g) ⇌ H2O(g) + CO(g)When equilibrium is reached, 0.49 mol of gaseous carbon monoxide is in the container. Based on this information, what is the value of the equilibrium constant, K?