Equilibrium Constant (Definition, Kc and Kp)

For  reaction a \(\ce{N2 + 3H2 <=> 2NH3}\), \(K_c = \)

For  reaction a \(\ce{2NH3 <=> N2 + 3H2}\), \(K_c = \)

The following concentrations were obtained for the formation of \(\ce{NH3 }\) from \(\ce{N2}\) and \(\ce{H2}\) at equilibrium at 500K. [\(\ce{N2}\)] = \(1.5 \times 10^{-2}\)M. [\(\ce{H2}\)] = \(3.0 \times 10^{-2}\) M and [\(\ce{NH3 }\)] = \(1.2 \times 10^{-2}\) M. Calculate equilibrium constant in nearest integer.

At equilibrium, the concentrations of \(\ce{N2}\)= \(3.0 \times 10^{-3}\) M , \(\ce{O2}\) = \(4.2 \times 10^{-3}\) M and \(\ce{NO}\)= \(2.8 \times 10^{-3}\) M in a sealed vessel at 800K. What will be \(K_c\) for the reaction \(\ce{N2(g) + O2(g) <=> 2NO(g)}\) in \(10^{-3}\) to the nearest integer?

Which of the following is/are always correct for a homogeneous gaseous equilibrium where \(K_c\) = Equilibrium constant (in terms of concentrations), and \(K_p\) = equilibrium constant,(in terms of pressure)?

For the equilibrium\(\ce{PCl5(g) <=> PCl3(g) + Cl2(g)}\):

For the equilibrium, \(\ce{2NO(g) + Cl2(g) 2NOCl(g)}\)

\(\ce{PCl5}\), \(\ce{PCl3}\) and \(\ce{Cl2}\) are at equilibrium at 500 K and having concentration 1.59M \(\ce{PCl3}\), 1.59M \(\ce{Cl2}\) and 1.41 M \(\ce{PCl5}\). Calculate \(K_c\) in \(10^{-2}\) for the reaction, \(\ce{PCl5 <=> PCl3 + Cl2}\) (nearest integer).