The reaction of bromine gas with chlorine gas, shown below, has a Kc of 7.20 at 200 oC. If a closed vessel was charged with the two reactants, each at an initial concentration of 0.50 M, what would be the equilibrium concentration of Cl2(g)?

Consider the equilibrium below A2g) + B2lg) 2AB(g) where Kc = 57.7 If the following are the initial concentrations, [A2] = 0.114 M, [B2]; = 0.114 M, and [AB]; = 0.212 M what is the equilibrium molarity of [ABleg? Type your answer in the space below without the units.

A 1.00-L flask was filled with 2.00 moles of gaseous SO2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.34 moles of gaseous NO was present. Assume that the reaction SO-(9) + NO2 (g) = SO; (g) + NO(9) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. K =

1) For the reaction shown below, at a particular time, the following concentrations are obtained: [CO] = 0.034 M, [CO2] = 3.6 x 10-17 M. Is this reaction at equilibrium? If not, which direction will the reaction proceed and what will the concentrations be at equilibrium? 2 CO (g) C (s) + CO2 (g) K = 7.7 x 10t5