Test: MCQs (One or More Correct Option): Equilibrium | JEE Advanced - JEE MCQ

The reaction is exothermic, hence increasing temperature will favour backward reaction (i.e. conc. of C₂H₄ increases) removing H₂ and adding C₂H₆ favours backward reaction.

According to Le-chatelier principle an increase in pressure always favours the reaction, where volume or moles decrease (i.e. reverse direction). As heat is added, i.e. reaction is endothermic and is supported in forward direction with increase in temperature.

At constant volume, concentrations do not change.

Introduction of an inert gas at constant pressure causes the equilibrium to shift in a direction in which number of moles increases. The forward reaction is further accelerated by increase in the quantity of substrate, i.e., PCl₅ and by the increase of space, i.e., volume of container.

A catalyst simply helps in attaining the equilibrium earlier.
Addition of inert gas has no effect on a reaction because in it Δn = 0.
This equilibrium is not based upon volume because in it  Δn = 0.
On increasing the amount of CO, K_C will decrease but it is constant at constant temperature, so for maintaining the constant value of K_C, the amount of CO₂ increases.

pH of 1 x 10^-8 M is below 7 because it is an acid.

K (Auto protolysis constant of water i.e. ionic product of water) increases with temperature. For half neutralisation of a weak acid by a weak base,

A buffer solution is prepared by mixing a weak acid/ base with salt of its conjugate base/acid.

Any solution of a weak acid and its salt with strong base acts as an acidic buffer solution.
If volume of HNO₃ solution added is less as compared to that of CH₃COONa solution, it results in the formation of an acidic buffer solution.

As ester hydrolysis is first order with respect [H⁺].

Hence enthalpy depends on temperature.

(C) K_eq depends only on temperature and not on Pressure.
(D) Enthalpy of reaction is independent of the catalyst.
Catalyst generaly changes activation energy.

Initially on increasing temperature rate of reaction will increase, so % yield will also increase with time. But at equilibrium % yield at high temperature (T₂) would be less than at T₁ as reaction is exothermic so the graph is