Chemical Equilibrium ( Chapter Test - Medical) - Class 12 MCQ

The conditions which favour the manufacture of ammonia by the reaction (Le-Chatelier’s principle)

1 mole of H₂ and 2 moles of I₂ are taken initially in a 5 litre vessel. If the number of moles of H₂ at equilibrium is 0.2, the number of moles of I₂ and HI, respectively at equilibrium would be

Consider the reaction  2H₂ + O₂ 2H₂O.

Which of the following correctly states the expression for the equilibrium constant for this reaction?

1.2 moles each of pure acetic acid and 1.2 moles of pure ethanol are subjected to esterification. At
equilibrium 0.4 moles of ester were found to have formed. The equilibrium constant for the reaction

At a rather high temperature the K_p values are computed as

What is the K_p for the reaction ?

Kc for a reaction A + 2B ⇔ D, is 0.64. What should be the concentration of B when it is in equilibrium with
equimolar quantities of A and D ?

In which of the following, K_p is not greater than K_c?

Given the equation,

Which combination of pressure and temperature should give the best yield of Z ?

The equilibrium constant K_p for the reaction 

is 16. If the volume of the container is reduced to one half of its original volume,the value of K_p for the reaction at the same temperature will be

The equilibrium constant for the given reaction is 100.

What is the equilibrium constant for the reaction given below

For the reaction,

the formation of Cl(g) is favoured at

In the system

doubling the mass of CaO will cause the equilibrium concentration of CO₂ to

In equilibrium constant expression, concentration of products is taken in/on the

Given the equilibrium reaction,

This reaction is studied by starting with equal amounts of A and B in a constant-volume vessel. Which of the following expressions will hold good ?

In a system

 if the equilibrium concentration of B increases to 8 times, it will cause the equilibrium concentration of C to change to

For the heterogeneous equilibrium

the temperature is given by

Given 

The equilibrium constant K₄ for the following reaction

may be given as