Equilibrium

The equilibrium constant for the reaction SO3(g) SO2(g) + 12O2(g) is Kc = 4.9 10-2. The value of Kc for the reaction given below 2SO2(g) + O2(g) 2SO3(g) is :

1. 49
2. 416
3. 41.6
4. 4.9

Ka for CH3COOH is 1.8 10-5 and Kb for NH4OH is 1.8 10-5. The pH of ammonium acetate solution will be .

Solubility of calcium phosphate (molecular mass, M) in water is W g per 100 mL at 25 . Its solubility product at 25 will be approximately.

1. 107 ( WM )3
2. 103 ( WM )5
3. 107 ( WM )5
4. 105 ( WM )5

For the given reaction, choose the correct expression of KC from the following :- Fe3+(aq) + SCN-(aq) (FeSCN)2+(aq)

1. KC = [ Fe3+][SCN-][ FeSCN2+]
2. KC = [ FeSCN2+][ Fe3+][SCN-]
3. KC = [ FeSCN2+]2[ Fe3+][SCN-]
4. KC = [ FeSCN2+][ Fe3+]2[SCN-]2

A(g) B(g) + C2(g) The correct relationship between KP, and equilibrium pressure P is

1. KP = 1/2P3/2(2+ )3/2
2. KP = 3/2P1/2(2+ )1/2(1- )
3. KP = 1/2P1/2(2+ )3/2
4. KP = 1/2P1/2(2+ )1/2

The pH at which Mg(OH)2 [ Ksp = 1 10-11 ] begins to precipitate from a solution containing 0.10 M Mg2+ ions is .

The pH of an aqueous solution containing 1 M benzoic acid (pKa = 4.20) and 1 M sodium benzoate is 4.5. The volume of benzoic acid solution in 300 mL of this buffer solution is mL. (given : log 2 = 0.3)

For the reaction N2O4(g) 2NO2(g), Kp = 0.492 atm at 300 K. Kc for the reaction at same temperature is 10-2. (Given : R = 0.082 L atm mol-1 K-1)

The following concentrations were observed at 500 K for the formation of NH3 from N2 and H2. At equilibrium ; [N2] = 2 10-2 M, [H2] = 3 10-2 M and [NH3] = 1.5 10-2 M. Equilibrium constant for the reaction is .

Given below are two statements : In the light of the above statements, choose the most appropriate answer from the options given below :

1. Both Statement I and Statement II are correct
2. Statement I is correct but Statement II is incorrect
3. Both Statement I and Statement II are incorrect
4. Statement I is incorrect but Statement II is correct