Equilibrium Tes...

Two flasks A and B of equal volume containing 1 mole and 2 mole of O₃ respectively, are heated to the same temperature. When the reaction 2O₃ →  3O₂ practically stops, then both the flasks shall have                       

A 10L container at 300K contains CO₂ gas at pressure of O.2 atm and an excess solid CaO (neglect the volume 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)   → CaO(s) + CO₂(g)

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 –

At 1400 K, K_c= 2.5x10 ⁺³ for the reaction CH₄(g) + 2H₂S(g) CS₂(g) + 4H₂(g) . A 10.0L reaction vessel at 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 → 2NO₂ (g) will be :

(the concentrations of N₂O₄ (g) and of NO (g) for which the following eaction will be at equilibrium will lie

In a basic aqueous solution chloromethane undergoes a substitution reaction in which Cl is replaced by OH^– as.

CH₃Cl (aq) + OH^- → CH₃OH(aq) + Cl(aq)

The equilibrium constant of above reaction C, =1 x 10'6. If a solution is prepared by mixing equal volumes of 0.1 M CH₃CI and 0.2 M NaOH (100% dissociated) then [OH^-] concentration at equilibrium in mixture will be:

For the chemical equilibrium,   
CaCO₃ (S) → CaO(s) + CO₂ (g)

ΔHf° can be determined from which one of the following plots ?

At a certain temperature the following equilibrium is established, CO(g) + N0₂(g) →  CO(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 C_c of the reaction is (Ba = 137)               

At temperature T, the compound AB₂ (g) dissociates according to the reaction, 2AB₂ (g)   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.

Equilibrium constant for the given reaction is C = 10²⁰ at temperature 300 K

A(s) +2B(aq)  2C (s) + D(aq.)K = 10²⁰

The equilibrium conc. of B starting with mixture of 1 mole of A and 1/3   mote/titre of B at 300 K is

10lt box contain O₃ and O₂ at equilibrium at 2000 K. The ΔG⁰ = –534.52  kJ at 8 atm equilibrium

pressure.The following equilibrium is present in the container 

2o₃(g)  3O₂ (g). the partial pressure of O₃ will be ( In 10 = 2.3, R = 8.3  J mol^-1 K^-1)

Solid ammonium carbamate dissociates to give ammonia and carbon dioxid as follows:

NH₂COONH₄(s) 2NH₅(g) + CO₂(g)

At equilibrium, ammonia is added such that partial pressures of NH₅ now equals the original total pressure. Calculate the ratio of the total pressures now to the original total pressure.

The reactions,   PCl₅ (g) PCl₅(g) + Cl₂(g) and Cl₂(g) CO₂(g) + Cl₂ (g) are simultaneously in equilibrium in an equilibrium box at constant volume. Afew  moles of   CO(g) are later introduced into the vessel. After some time, the new  equilibrium concentration of      

In the Haber process for the industrial manufacture of ammonia involving the  reaction,   atm pressure in the presence of a catalyst a temperature of about 500°C is used. This is considered as optimum temperature for the process because     

For the equilibrium of the reaction   ,k_P for the reaction at total pressure of P is:

What is the minimum mass of CaC0₅ (s), below which it decomposes completely, required to establish equilibrium in a 6.50 litre container for the reaction : [ K_C = mole/litre]

CaCO₃ (s)  CaO(s) + CO₂(g)

The value of k_p for the reaction at 27°C

is '1 atom'. At equilibrium in a closed container partial pressure of BrCI gas is 0.1 atm and at this temperature the vapour pressure of Br₂(l) is also 0.1 atm. Then what will be minimum moles of Br₂(l) to be added to 1 mole of C1₂ , initially, to get above equilibrium situation :

5 mol PCI₃(g) and one mole N₂ gas is placed in a closed vessel. At equilibrium PCI₅(g) decomposes 20% and total pressure in to the container is found to be 1 atm. The k_P for equilibrium 

Degree of association can be defined as the number of moles of a particular substance associated per mole of the substance taken.               

For example : If out of 10 mole of N₂ , 3 mol of N₂ combine with H₂ to form NHL. then degree of association of N₂ = 0.3.Consider the equilibrium situation :  N₂(g) + 3H₂(g)   2NH₃(g)

 Initially N₂ & H₂ were mixed in 1 : 3 molar ratio and after long time the mean molar mass of the mixture was  found to be 34/3g. The degree of association of N₂ is               

Attainment of the equilibrium A(g)  2C(g) +B(g) gave the gave the followeing graph. Find the correct option. (% dissociation = fraction dissociated x 100)