The Initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and use it to determine the direction in which each system will proceed to reach equilibrium. Write??lfthe reactions shifts to the right towards products or \"L-ERShits left towards reactants. A(NO 1.00 M, (CL) 1.00 M, 2 NOg)+ C22 NOC 0.00 M;K 4.6x 10 B.(SO.)-2.00 M, (SO.)-2.00 M, (O.)-2.00 M; K 0.230 2 S032 S02 ( O2 C. (N)-0.100 M, (O)-0.200 M, (NO)-1.00 M; K 0.050 N2 (g) + O2 (g) ++ 2 NO(g) 74 of 104 Solution Qc=[products]/[reactants] If Qc=Kc then the reaction is at equilibrium If Qc<Kc then the reaction will shift right to reach equilibrium If Qc>Kc then the reaction will shift left to reach equilibrium i will caculate one you calculate remaining (a) 2NO (g) + Cl2 (g) <-> 2NOCl(g) Qc = [NOCl]^2/ [NO]^2 [Cl] = 0.0 (since[NOCl]=0) Qc<Kc then the reaction will shift right to reach equilibrium similarly you calculate remaining keep remember that othe thingd given in atm dont bother take it directly .