The initial concentrations or pressures of reactants and products are given for

Question

The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (a) 2NH3 (g) N2 (g) + 3H2 (g) Kc = 17; [NH3] = 0.50 M, [N2] = 0.15 M, [H2] = 0.12 M

(b) 2NH3 (g) N2 (g) + 3H2 (g) KP = 6.8 × 104 ; initial pressures: NH3 = 2.00 atm, N2 = 10.00 atm, H2 = 10.00 atm

(c) 2SO3 (g) 2SO2 (g) + O2 (g) Kc = 0.230; [SO3] = 2.00 M, [SO2] = 2.00 M, [O2] = 2.00 M

(d) 2SO3 (g) 2SO2 (g) + O2 (g) KP = 6.5 atm; initial pressures: SO2 = 1.00 atm, O2 = 1.130 atm, SO3 = 0 atm

Explanation / Answer

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) 2NH3 (g) N2 (g) + 3H2 (g

Qc = [N2] [H2]3 / [NH3]2

= [0.15] x [0.12]3 / [0.5]2

= 0.0002592 / 0.25

= 0.001

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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