Equilibrium Constant

What is the expression for the equilibrium constant $K_c$ for the reaction $aA + bB \rightleftharpoons cC + dD$?

If the equilibrium constant $K_c$ for a reaction is 0.5, what does this indicate about the concentrations of products and reactants?

For the reaction $N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$, what is the expression for the equilibrium constant ?

Which of the following changes will not affect the value of the equilibrium constant $K_c$?

For the endothermic reaction $A + B \rightleftharpoons C + D$, if the temperature is increased, what happens to the equilibrium constant $K_c$?

What is the value of the equilibrium constant $K_c$ for a reaction at equilibrium if the concentrations are $[A] = 0.2$, $[B] = 0.5$, , and for the reaction ?

If the equilibrium constant $K_p$ is known to be 2.0 for the reaction $2NO(g) \rightleftharpoons N_{2}(g) + O_{2}(g)$, what will be the value of ? (Assume ideal gas behavior)

In the equilibrium reaction $2SO_{2}(g) + O_{2}(g) \rightleftharpoons 2SO_{3}(g)$, what happens to the equilibrium constant if the volume of the system is decreased?