Equilibrium Constant

For the reaction $aA + bB \rightleftharpoons cC + dD$, the equilibrium constant $K_c$ is expressed as what?

If the equilibrium constant $K_c$ for a reaction is 10, what can be inferred about the position of equilibrium?

For the reaction $N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$, if $K_p = 0.5$, what is the relationship between products and reactants at equilibrium?

What effect does increasing the temperature have on the equilibrium constant $K_c$ for an exothermic reaction?

The equilibrium constant $K_c$ for the reaction $2SO_{2}(g) + O_{2}(g) \rightleftharpoons 2SO_{3}(g)$ is 4. What is $K_c$ for the reverse reaction?

In a certain reaction, the equilibrium constant $K_c$ is expressed in terms of concentrations. How does $K_c$ change if the concentrations of all species are doubled?

For the equilibrium $N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$, if $[NH_{3}] = 0.1$ M, $[N_{2}] = 0.2$ M, and $[H_{2}] = 0.3$ M, what is $K_c$?

For the reaction $2NO(g) + O_{2}(g) \rightleftharpoons 2NO_{2}(g)$, if the reaction is endothermic and $K_c$ increases with temperature, what does this indicate?

If the equilibrium constant $K_c$ for a reaction is 0.1 at 25 degrees Celsius, what does this suggest about the reaction?

In the reaction $A(g) \rightleftharpoons B(g)$, if the concentration of $A$ decreases, what happens to $K_c$?