A precipitate is formed if the ionic product is __________?
A precipitate is formed if the ionic product is __________?
Greater than the solubility product
Lesser than the solubility product
Equal to solubility product
Independent of solubility product
The Correct Option is A
Solution and Explanation
The correct option is (A): Greater than the solubility product
Top Questions on Law Of Chemical Equilibrium And Equilibrium Constant
For the reaction A(g) $\rightleftharpoons$ 2B(g), the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K.
[Given: R = 0.0831 atm $mol^{–1} K^{–1}$]
$K_p$ for the reaction at 1000 K is:- NEET (UG) - 2025
- Chemistry
- Law Of Chemical Equilibrium And Equilibrium Constant
The equilibrium constant for decomposition of $ H_2O $ (g) $ H_2O(g) \rightleftharpoons H_2(g) + \frac{1}{2} O_2(g) \quad (\Delta G^\circ = 92.34 \, \text{kJ mol}^{-1}) $ is $ 8.0 \times 10^{-3} $ at 2300 K and total pressure at equilibrium is 1 bar. Under this condition, the degree of dissociation ($ \alpha $) of water is _____ $\times 10^{-2}$ (nearest integer value). [Assume $ \alpha $ is negligible with respect to 1]
- JEE Main - 2025
- Chemistry
- Law Of Chemical Equilibrium And Equilibrium Constant
- Higher yield of NO in the reaction
N$_2$ (g) + O$_2$ (g) $\rightarrow$ 2NO (g)
can be obtained at [$\Delta H$ of the reaction = +180.7 kJ mol$^{-1}$]- NEET (UG) - 2025
- Chemistry
- Law Of Chemical Equilibrium And Equilibrium Constant
- At equilibrium, the concentration of \( N_2 = 5 \times 10^{-3} \, \text{M} \), \( O_2 = 2.8 \times 10^{-3} \, \text{M} \), and \( NO = 1.4 \times 10^{-3} \, \text{M} \) in a sealed vessel at 800 K. What is the value of \( K_c \) for the reaction at the same temperature? \[ N_2(g) + O_2(g) \rightleftharpoons 2NO(g) \]
- KEAM - 2025
- Chemistry
- Law Of Chemical Equilibrium And Equilibrium Constant
Consider the following gas phase dissociation, PCl$_5$(g) $\rightleftharpoons$ PCl$_3$(g) + Cl$_2$(g) with equilibrium constant K$_p$ at a particular temperature and at pressure P. The degree of dissociation ($\alpha$) for PCl$_5$(g) is
PCl$_5$(g) $\rightleftharpoons$ PCl$_3$(g) + Cl$_2$(g)- WBJEE - 2025
- Chemistry
- Law Of Chemical Equilibrium And Equilibrium Constant
Questions Asked in SRMJEEE exam
The molar conductivities at infinite dilution for Na2SO4,K2S04,KCl, HCl and HCOONa at 300K are 260, 308, 150, 426, and 105 S cm2 mol-1, respectively. What will be A+m for formic acid in the same unit?
- SRMJEEE - 2023
- Electrochemistry
- The current of 2A passing through a coil of 100 turns gives rise to a magnetic flux of 5 x 10-5 Wb/turn, the magnetic energy associated with the coil is _________ J
- SRMJEEE - 2023
- Electromagnetic induction
Markovnikov reaction is a
- SRMJEEE - 2023
- Organic Chemistry - Some Basic Principles and Techniques
Calculate the Reynold’s number for a liquid of density 1 g/cm3, viscosity 8 x 10-4 Pa.s flowing at 0.5 m/s through a pipe of diameter 4 cm?
- SRMJEEE - 2023
- Fluid Mechanics
Which of the following statement is true for aqueous solution of 0.1 M urea, 0.2 M glucose nad 0.3 M sucrose
- SRMJEEE - 2023
- Biomolecules
Concepts Used:
Law of Chemical Equilibrium
Law of Chemical Equilibrium states that at a constant temperature, the rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants each raised to a power equal to the corresponding stoichiometric coefficients as represented by the balanced chemical equation.
Let us consider a general reversible reaction;
A+B ↔ C+D
After some time, there is a reduction in reactants A and B and an accumulation of the products C and D. As a result, the rate of the forward reaction decreases and that of backward reaction increases.
Eventually, the two reactions occur at the same rate and a state of equilibrium is attained.
By applying the Law of Mass Action;
The rate of forward reaction;
Rf = Kf [A]a [B]b
The rate of backward reaction;
Rb = Kb [C]c [D]d
Where,
[A], [B], [C] and [D] are the concentrations of A, B, C and D at equilibrium respectively.
a, b, c, and d are the stoichiometric coefficients of A, B, C and D respectively.
Kf and Kb are the rate constants of forward and backward reactions.
However, at equilibrium,
Rate of forward reaction = Rate of backward reaction.
Kc is called the equilibrium constant expressed in terms of molar concentrations.
The above equation is known as the equation of Law of Chemical Equilibrium.