The hydrogen ion concentration of a 10^-8 M HCl aqueous solution at 298 K (K_w = 10^-14) is:

(1) 1.0×10^-6 M

(2) 1.0525 x 10^-7 M

(3) 9.525 x 10^-8 M

(4) 1.0×10^-8 M

The equilibrium constant for the reaction 

$N{H}_{4}N{O}_2\left(s\right)$$N_2\left(g\right) + 2H_{2}O\left(g\right)$ is given by

(1) $\frac{\left[N_2\right]\left[H_{2}O\right]}{\left[N{H}_{4}N{O}_2\right]}$

(2) $\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\mathrm{O}\right]}^2$

(3) $\frac{\left[H_{2}O\right]}{\left[N{H}_{4}N{O}_2\right]}$

(4) $\frac{\left[N_2\right]}{\left[N{H}_{4}N{O}_2\right]}$

Two flasks A and B of equal volume containing 1 mole and 2 mole of O₃ respectively, are heated to the sametemperature. When the reaction 2O₃ $\underset{}{\overset{}{\leftrightharpoons }}$3O₂ practically stops, then both the flasks shall have

(1) the same ratio [O₂] /[O₃]

(2) the same ratio : [O₂]³/²/[O₃]

(3) only O₂

(4) the same time to reach equilibrium

A 10L container at 300K contains CO₂ gas at pressure of 0.2 atm and an excess solid CaO (neglect thevolume of solid CaO). The volume of container is now decreased by moving the movable piston fitted in the container. What will be the maximum volume of container when pressure of CO₂ attains its maximum value given that CaCO₃ (s) $\underset{}{\overset{}{\leftrightharpoons }}$ CaO(s) + CO₂(g)K_ph = 0.800 atm

1. 5 L

2. 2.5 L

3. 1 L

4. The information is insufficient.

An equilibrium mixture at 700 K of 0.50 M N₂, 3.00 M H₂ and 2.00 M NH₃ is present in a container. Now if this equilibrium is disturbed by adding N₂ so that its concentration becomes 1.50 M just after addition then which of the following graphs represents the above situation more appropriately –

(1)

(2)

(3)

(4)

At 1400 K, K_c= 2.5x10^-3 for the reaction CH₄(g) + 2H₂S(g) $\underset{}{\overset{}{\rightleftharpoons }}$ CS₂(g) + 4H₂(g). A 10.0L reaction vesselat 1400 K contains 2.00 mole of CH₄, 3.0 mol of CS₂, 3.0 mole of H₂ and 4.0 mole of H₂S. Then

The graph which will be representing all the equilibrium concentrations for the reaction N₂O₄(g) $\underset{}{\overset{}{\rightleftharpoons }}$ 2NO2 (g) will be : (the concentrations of N₂O₄ (g) and of NO (g) for which the following reaction will be at equilibrium will lie:

(1)       

(2)        

(3)         

(4)      

For the chemical equilibrium, CaCO₃(s) $\stackrel{}{\rightleftharpoons }$ CaO(s) + CO₂ (g) ΔH_f° can be determined from which one of the following plots ?

(1)  

(2) 

(3) 

(4) 

At a certain temperature the following equilibrium is established, CO(g) + N0₂(g) $\stackrel{}{\rightleftharpoons }$ CO₂(g)+ NO(g)One mole of each of the four gas is mixed in one litre container and the reaction is allowed to reach equilibrium state. When excess of baryta water (Ba(OH)₂) is added to the equilibrium mixture, the weight of white ppt (BaCO₃) obtained is 236.4 gm. The equilibrium constant K_c of the reaction is (Ba = 137)

(1) 1.2

(2) 2.25

(3) 2.1

(4) 3.6

At temperature T^, the compound AB₂ (g) dissociates according to the reaction, 2AB₂ (g) $\stackrel{}{\rightleftharpoons }$ 2 AB(g) + B₂(g). With a degree of dissociation x^, which is small compared with unity. Deduce the expression for x in terms of the equilibrium constant, K_p and the total pressure, P.

(1) $\mathrm{x} =\hspace{0.17em}{\left[\frac{{\displaystyle 2{\mathrm{K}}_{\mathrm{p}}}}{{\displaystyle \mathrm{P}}}\right]}^{–1/3}$

(2) $\mathrm{x} =\hspace{0.17em}{\left[\frac{{\displaystyle {\mathrm{K}}_{\mathrm{p}}}}{{\displaystyle \mathrm{P}}}\right]}^{1/3}$

(3) $\mathrm{x} =\hspace{0.17em}{\left[\frac{{\displaystyle {\mathrm{K}}_{\mathrm{p}}}}{{\displaystyle \mathrm{2P}}}\right]}^{1/3}$

(4) $\mathrm{x} =\hspace{0.17em}{\left[\frac{{\displaystyle 6{\mathrm{K}}_{\mathrm{p}}}}{{\displaystyle 3\mathrm{P}}}\right]}^{1/3}$