Chemical Equilibrium

What is the equilibrium expression for the reaction P₄ (s) + 5O₂ $\leftrightharpoons$ P₄O₁₀ (s)?

The equilibrium constant for the reaction N₂(g) + O₂(g) $\leftrightharpoons$ 2NO(g) at temperature T is 4 $\times$ 10⁻⁴. The value of K_c for the reaction NO(g) $\leftrightharpoons$ $1 \over 2$N₂ (g) + $1 \over 2$O₂ (g) at the same temperature is :

For the reaction CO (g) + (1/2) O₂ (g) $\leftrightharpoons$ CO₂ (g), K_p/K_c is :

For the reaction equilibrium N₂O₄ (g) $\leftrightharpoons$ 2NO₂ (g) the concentrations of N₂O₄ and NO₂ at equilibrium are 4.8 $\times$ 10⁻² and 1.2 $\times$ 10⁻² mol L⁻¹ respectively. The value of K_c for the reaction is

For the reaction 2NO₂ (g) $\leftrightharpoons$ 2NO (g) + O₂ (g), (K_c = 1.8 $\times$ 10⁻⁶ at 184^oC) (R = 0.0831 kJ/(mol. K)) When K_p and K_c are compared at 184^oC , it is found that :

An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm. Pressure. Ammonium hydrogen sulphide decomposes to yield NH₃ and H₂S gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm. The equilibrium constant for NH₄HS decomposition at this temperature is :

Phosphorus pentachloride dissociates as follows, in a closed reaction vessel PCl₅ (g) $\leftrightharpoons$ PCl₃ (g) + Cl₂ (g) If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PCl₅ is x, the partial pressure of PCl₃ will be

The equilibrium constant for the reaction SO₃ (g) $\leftrightharpoons$ SO₂ (g) + $1 \over 2$ O₂ (g) is K_c = 4.9 $\times$ 10^–2. The value of K_c for the reaction 2SO₂ (g) + O₂ (g) $\leftrightharpoons$ 2SO₃ (g) will be :

The equilibrium constants K_P1 and K_P2 for the reactions X $\leftrightharpoons$ 2Y and Z $\leftrightharpoons$ P + Q, respectively are in the ratio of 1 : 9. If the degree of dissociation of X and Z be equal then the ratio of total pressure at these equilibria is :

For the following three reactions a, b and c, equilibrium constants are given: a. CO (g) + H₂O (g) $\leftrightharpoons$ CO₂(g) + H₂ (g) ; K₁ b. CH₄ (g) + H₂O (g) $\leftrightharpoons$ CO(g) + 3H₂ (g) ; K₂ c. CH₄ (g) + 2H₂O (g) $\leftrightharpoons$ CO₂(g) + 4H₂ (g) ; K₃

In aqueous solution the ionization constants for carbonic acid are K₁ = 4.2 x 10^–7 and K₂ = 4.8 x 10^–11 Select the correct statement for a saturated 0.034 M solution of the carbonic acid.

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

The equilibrium constant (K_C) for the reaction N₂(g) + O₂(g) $\to$ 2NO(g) at temperature T is 4 $\times$ 10^–4. The value of K_C for the reaction, NO(g) $\to$ 1/2N₂(g) + 1/2O₂(g) at the same temperature is :

For the reaction SO₂ (g) + ${1 \over 2} O_2(g) \leftrightharpoons$ SO₃(g). if K_P = K_C(RT)^x where the symbols have usual meaning then the value of x is: (assuming ideality)

The standard Gibbs energy change at 300 K for the reaction 2A $\leftrightharpoons$ B + C is 2494.2 J. At a given time, the composition of the reaction mixture is [A] = 1/2, [B] = 2 and [C] = 1/2. The reaction proceeds in the: [R = 8.314 J/K/mol, e = 2.718]

The equilibrium constant at 298 K for a reaction A + B $\leftrightharpoons$ C + D is 100. If the initial concentration of all the four species were 1M each, then equilibrium concentration of D (in mol L^–1) will be:

A solid XY kept in an evacuated sealed container undergoes decomposition to form a mixture of gases X and Y at temperature T. The equilibrium pressure is 10 bar in this vessel. K_p for this reaction is :

At a certain temperature in a $5$ $L$ vessel, 2 moles of carbon monoxide and 3 moles of chlorine were allowed to reach equilibrium according to the reaction,          CO + Cl₂ $\rightleftharpoons$ COCl₂ At equilibrium, if one mole of CO is present then equilibrium constant (K_c) for the reaction is :

In which one of the following equilibria, K_p $\ne$ K_C ?