If the equilibrium concentrations are 1.33 M A, 2.03 M B, and 2.39 M C, calculate the value of the equilibrium constant of the reverse reaction. Kreverse = 1.1292 Incorrect

Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?

. Suppose that for the reaction PCl5(g)PCl3(g)+Cl2(g)it is determined, at a particular temperature. that the equilibrium concentrations are [PCl5(g)]=0.0711M,[PCl3(g)]=0.0302M, and [Cl2(g)]=0.0491M. Calculate the value of K for he reaction at this temperature.

At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?