Why is it useful to compare Q with `K`?
What is the situation when
a. `Q=K` b. `QltK` c.` QgtK`?

If a = i + j, b = j + k and c = i + k then a unit vector in the direction of a - 2b + 3c is

Mass action ratio or reaction quotient Q for a reaction can be calculated using the law of mass action A(g)+B(g) harr C(g) + D(g) Q=([C][D])/([A][B]) . The value of Q decides whether the reaction is at equilibrium or not. At equilibrium, Q = K. For non equilibrium process, Q ne K . When Q gt K , reaction will favour backward direction and when Q lt K , it will favour forward direction. For the reaction : 2A + B harr 3C at 298 K, K_c = 49 A 3L vessel contains 2,1 and 3 moles of A, B and C respectively. The reaction at the same temperature:

Mass action ratio or reaction quotient Q for a reaction can be calculated using the law of mass action A(g)+B(g) harr C(g) + D(g) Q=([C][D])/([A][B]) . The value of Q decides whether the reaction is at equilibrium or not. At equilibrium, Q = K. For non equilibrium process, Q ne K . When Q gt K , reaction will favour backward direction and when Q lt K , it will favour forward direction. In a reaction mixture containing H_2 , N_2 and NH_3 at partial pressure of 2 atm, and 3 atm respectively, the value of K_p at 725 K is 4.28 xx 10^(-5) atm^(-2) . In which direction the net reaction will go ? N_(2(g)) + 3H_(2(g)) harr 2NH_(3(g))