The Initial concentrations or pressures of reactants and products are.docx

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This document provides the initial concentrations of reactants and products for three chemical reaction systems and asks to determine the direction each reaction will proceed to reach equilibrium. 1) The first reaction involves NO, Cl2, and NOCl. The reaction quotient is calculated and found to be less than the equilibrium constant, so the reaction will shift right towards the products. 2) For the second reaction involving SO2, S03, and O2, the student is asked to calculate the reaction quotient and determine the direction. 3) The third reaction involves N2, O2, and NO. Again, the student should calculate the reaction quotient and state which way the reaction will shift to reach equilibrium.

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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

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