At equilibrium, the concentration of : N_2=3.0xx10^(-3) M, O_2=4.2xx10^(-3) M and NO=2.8xx10^(-3) M in a sealed vessel at 800 K. What will be K_c for the reaction N_(2(g)) + O_(2(g)) hArr 2NO_((g))

At equilibrium, the concentration of : N_2=3.0xx10^(-3) M, O_2=4.2xx10

1.	At equilibrium, the concentration of : N_2=3.0xx10^(-3) M, O_2=4.2xx10^(-3) M and NO=2.8xx10^(-3) M in a sealed vessel at 800 K. What will be K_c for the reaction N_(2(g)) + O_(2(g)) hArr 2NO_((g))
Answer» Solution :`{:("REACTION:" ,N_(2(g)) + , O_(2(g))hArr , 2NO_((g))),("Concentration at equilibrium:" , 3.0xx10^(-3)M, 4.2xx10^(-3)M,2.8xx10^(3)M):}` Equilibrium CONSTANT of reaction is `K_c`, `K_c=[NO]^2/([N_2][O_2])=(2.8xx10^(-3)M)^2/((3.0xx10^(-3)M)(4.2xx10^(-3)M))` = 0.6222