Equilibrium
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New answer posted
3 months agoContributor-Level 10
This is a Long Answer Type Questions as classified in NCERT Exemplar
Ans: The values of Kc and Qc are itself sufficient to explain the direction of reaction and less than or greater than one another decides the direction in which reaction will proceed as follows-
(i) As Qc < Kc, the reaction proceeds in the forward direction.
(ii) If Qc > Kc, the reaction will proceed in the direction of reactants (reverse reaction).
(iii) If Qc = Kc, no net reaction occurs.
New answer posted
4 months agoContributor-Level 10
(i) Le Chatelier's principle states that the change in any factor such as temperature, pressure, concentration, etc. will cause the equilibrium to shift in such a direction so as to reduce or counteract the effect of the change.
(ii) (a) On adding Fe2O3 (s), the equilibrium will remain unaffected.
(b) By removing CO2 (g), the equilibrium will be shifted in the forward direction.
(c) By removing CO (g), the equilibrium will be shifted in the backward direction.
New answer posted
4 months agoContributor-Level 10
Whenever equilibrium is disturbed by change in the concentration, pressure or volume, the composition of the equilibrium mixture changes because the reaction quotient, Qc no longer equals the equilibrium constant, Kc. However, when a change in temperature occurs, the value of equilibrium constant, Kc is changed.
In general, the temperature dependence of the equilibrium constant depends on the signoff ΔH for the reaction.
- The equilibrium constant for an exothermic reaction (negative ΔH) decreases as the temperature increases.
- The equilibrium constant for an endothermic reaction (positive ΔH)increases as the temperature increases. Temper
New answer posted
4 months agoContributor-Level 10
If the volume is kept constant and an inert gas such as argon is added which does not take part in the reaction, the equilibrium remains undisturbed. It is because the addition of an inert gas at constant volume does not change the partial pressures or the molar concentrations of the substance involved in there action. The reaction quotient changes only if the added gas is a reactant or product involved in the reaction.
New answer posted
4 months agoContributor-Level 10
The intensity of the red colour becomes constant on attaining equilibrium. This equilibrium can be shifted in either forward or reverse directions depending on adding a reactant or a product. The equilibrium can be shifted in the opposite direction by adding reagents that remove Fe3+or SCN– ions. For example, oxalic acidH2C2O4), reacts with Fe3+ ions to form testable complex ion [Fe (C2O4)3]3–, thus decreasing the concentration of free Fe3+ (aq).In accordance with the Le Chatelier's principle, the concentration stress of removed Fe3+ is relieved by dissociation of [Fe (SCN)]2+ to replenish the Fe3+ions. Because the concentration of
New answer posted
4 months agoContributor-Level 10
This is because at lower pH, the concentration of the anion decreases due to its protonation. This in turn increase the solubility of the salt so that Ksp = Qsp.
New answer posted
4 months agoContributor-Level 10
The solutions which resist change in pH on dilution or with the addition of small amounts of acid or alkali are called Buffer Solutions.
- Its pH does not change on the addition of small amount of acid or base.
- Its pH does not change on dilution or standing.
New answer posted
4 months agoContributor-Level 10
It is product of molar concentration of ion raised to the power of number of ions produced per compound in saturated solution.
Solubility of electrolyte decreases due to common ion effect.
New answer posted
4 months agoContributor-Level 10
Equilibrium is a state at which rate of forwarding reaction is equal to the rate of backward reaction. The equilibrium between ions and unionised molecules is called ionic equilibrium.
New answer posted
4 months agoContributor-Level 10
A catalyst does not affect the equilibrium composition of a reaction mixture. Catalysts influence the rate of both forward and backward reactions equally.
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