Equilibrium

37.8 g N2O5 was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 500 K 2N2O5(g) 2N2O4(g) + O2(g) The total pressure at equilibrium was found to be 18.65 bar. Then, Kp = 10-2 [nearest integer] Assume N2O5 to behave ideally under these conditions. Given: R = 0.082 bar L mol-1 K-1

For the reaction, H2(g)+I2(g) 2HI(g) Attainment of equilibrium is predicted correctly by :

1. [figure]
2. [figure]
3. [figure]
4. [figure]

Which of the following happens when NH4OH is added gradually to the solution containing 1 M A2+ and 1M B3+ ions? Given : Ksp [A(OH)2] = 9 10-10 and Ksp [B(OH)3] = 27 10-18 at 298 K.

1. A(OH)2 will precipitate before B(OH)3
2. A(OH)2 and B(OH)3 will precipitate together
3. Both A(OH)2 and B(OH)3 do not show precipitation with NH4OH
4. B(OH)3 will precipitate before A(OH)2

If 1 mM solution of ethylamine produces pH=9, then the ionization constant (Kb) of ethylamine is 10-x. The value of x is (nearest integer). [The degree of ionization of ethylamine can be neglected with respect to unity.]

pH of water is 7 at 25 C. If water is heated to 80 C, it's pH will :

1. Decrease
2. Remains the same
3. Increase
4. H+ concentration increases, OH- concentration decreases

Consider the reaction X2Y(g) X2(g) + 12Y2(g) The equation representing correct relationship between the degree of dissociation (x) of X2Y(g) with its equilibrium constant Kp is . Assume x to be very very small.

1. x = [3] KpP
2. x = [3] Kp2P
3. x = [3] 2 Kp2P
4. x = [3] 2KpP

A vessel at 1000 K contains CO2 with a pressure of 0.5 atm. Some of CO2 is converted into CO on addition of graphite. If total pressure at equilibrium is 0.8 atm, then Kp is :

1. 0.18 atm
2. 0.3 atm
3. 3 atm
4. 1.8 atm

The molar solubility(s) of zirconium phosphate with molecular formula ( Zr4+ )3 ( PO43- )4 is given by relation :

1. ( Ksp5348 )1/6
2. ( Ksp8435 )1/7
3. ( Ksp6912 )1/7
4. ( Ksp9612 )1/3

For a sparingly soluble salt AB2, the equilibrium concentrations of A2+ ions and B- ions are 1.2 10-4 M and 0.24 10-3 M, respectively. The solubility product of AB2 is :

1. 0.069 10-12
2. 0.276 10-12
3. 6.91 10-12
4. 27.65 10-12

For the given hypothetical reactions, the equilibrium constants are as follows : X Y; K1 = 1.0 Y Z; K2 = 2.0 Z W; K3 = 4.0 The equilibrium constant for the reaction X W is

1. 12.0
2. 8.0
3. 6.0
4. 7.0