Explanation
Δng = 2 – 3 = 1
∴ Kp = Kc (RT)–1 = Kc / RT
Kp = Kc when Δng = 0.
K = Product of eqm. Constants of step reactions.
As K decreases with increase of temperature, the reaction is exothermic.
Apply law of chemical equilibrium
Apply law of chemical eqm, taking [solid] = 1.
The amount of A reacted is double the amount of B reacted.
K depends upon units of concentrations when np ≠ nr
(d) is not an equilibrium reaction, being irreversible.
On adding more PCl5, equilibrium shifts forward.
Pressure has no effect when np = nr
Endothermic reaction is favoured by increase of temp.
Conversion of graphite to diamond is an endothermic reaction. All other reactions are exothermic (Note that decomposition of ozone is also exothermic).
Concentrations of reactants and products at equilibrium are same even in the presence of catalyst.
Forward reaction will be favoured by increase of temp.
Reaction is exothermic with np < nr
Reaction is exothermic with np = nr .Apply Le Chatelier principle.
If CO2 escapes, equilibrium will shift in the backward direction
Eqm. Const. Of a reaction depends only on temperature.
(b) By law of chemical equilibrium
Vapours and liquid are at the same temperature
(d) By law of chemical equilibrium.
Decrease of K with rise of temp. means that the forward reaction is exothermic or the backward reaction (formation of HI) is endothermic. As the given reaction is exothermic, energy of HI is greater or stability is less than H2 and I2.
As np = nr, equilibrium will not be disturbed by pressure.
Greater the value of K, more it goes towards completion.
Doubling the volume means decrease of pressure. It will shift to right for reaction in which np > nr
Eqm. Shifts backward by Le Chatelier principle.
np ≠ nr and K changes with temp. Hence Ans. Is (a).
(a) by Le Chatelier principle.
(a) is correct because concentrations of H2 and N2 decrease while that of NH3 increases with time and after equilibrium, all of them remain constant.
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