For the gas phase reaction :
carried out in a vessel, the equilibrium concentration of C2H4 can be increased by :
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.
When NaNO3 is heated in a closed vessel, oxygen is liberated and NaNO2 is left behind. At equilibrium.
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.
The equilibrium :
is attained at 25ºC in a closed container and an inert gas, helium is introduced. Which of the following statements are correct?
At constant volume, concentrations do not change.
For the reaction :
The forward reaction at constant temperature is favoured by
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.
For the reaction at a given temperature the equilibrium amount of CO2(g) can be increased by
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, KC will decrease but it is constant at constant temperature, so for maintaining the constant value of KC, the amount of CO2 increases.
Which of the following statements(s) is (are) correct?
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 can be prepared from a mixture of
A buffer solution is prepared by mixing a weak acid/ base with salt of its conjugate base/acid.
Aqueous solutions of HNO3 , KOH, CH3COOH and CH3COONa of identical concentrations are provided. The pair(s) of solutions which form a buffer upon mixing is(are)
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.
The initial rate of hydrolysis of methyl acetate (1M) by a weak acid (HA, 1M) is 1/100th of that of a strong acid (HX, 1M), at 25°C. The Ka of HA is
As ester hydrolysis is first order with respect [H+].
The Ksp of Ag2CrO4 is 1.1 × 10–12 at 298 K. The solubility (in mol/L) of Ag2CrO4 in a 0.1 M AgNO3 solution is
The thermal dissociation equilibrium of CaCO3(s) is studied under different conditions
For this equilibrium, the correct statement(s) is(are)
Hence enthalpy depends on temperature.
(C) Keq depends only on temperature and not on Pressure.
(D) Enthalpy of reaction is independent of the catalyst.
Catalyst generaly changes activation energy.
The %yield of ammonia as a function of time in the reaction is given below
If this reaction is conducted at (P, T2), with T2 > T1, the %yield of ammonia as a function of time is represented by
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