List of top Chemistry Questions on Law Of Chemical Equilibrium And Equilibrium Constant

An equilibrium mixture taken in 2 litre vessel of the reaction: \[ \mathrm{2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)} \] has 4 moles of $\mathrm{SO_2}$, 3 moles of $\mathrm{O_2}$ and 6 moles of $\mathrm{SO_3}$ then the value of equilibrium constant $(K_c)$ will be:
Kc for the reaction A(g) + 2B(g) \(\rightleftharpoons\) C(g) + 2D(g) is 4.0 at 300 K. What is the value of K'c for the reaction, 2C(g) + 4D(g) \(\rightleftharpoons\) 2A(g) + 4B(g) at 300 K?
For the homogeneous equilibrium \(N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}\), the equilibrium constants \(K_P\) and \(K_C\) are related as:
Which one of the following conditions will favour maximum formation of the product in the reaction, \( A_{2}(g) + B_{2}(g) \rightleftharpoons X_{2}(g) \), \( \Delta_r H = -x \,\text{kJ} \):
For the equilibrium,
\( 2\text{A}_{(g)} \rightleftharpoons 2\text{B}_{(g)} + 2\text{C} \)
the value of \( K_p \) is 0.1662 atm at 1000 K. The value of \( K_c \) at the same temperature is ( \( R = 0.0831 \) )
Predict expression for \( \alpha \) in terms of \( K_{eq} \) and concentration
C: \( A_2B_3 \, (aq) \rightleftharpoons 2A^{3+} (aq) + 3B^{2-} (aq) \)
For a given reaction at 400 K (R = 0.082 atm-L/mol-K) \[ xA \longleftrightarrow yB \] Given (i) \(K_f = 0.82\), \(K_c = 25.7\)
(ii) \(K_f = 8.2\), \(K_c = 0.25\)
Then which will be the correct combination of x & y for above set (i) & set (ii) data?
Consider the following gaseous equilibrium in a closed container of volume $V$ at temperature $T$:
P$_2$(g) + Q$_2$(g) $\rightleftharpoons$ 2PQ(g)
Initially, 2 moles each of P$_2$(g), Q$_2$(g) and PQ(g) are present at equilibrium. One mole each of P$_2$ and Q$_2$ are added. The number of moles of P$_2$, Q$_2$ and PQ at the new equilibrium respectively are
The plot of \(\log_{10}K\) vs \(\frac{1}{T}\) gives a straight line. The intercept and slope respectively are (where \(K\) is equilibrium constant).
Consider the gas phase dissociation, PCl$_5$(g) $\rightleftharpoons$ PCl$_3$(g) + Cl$_2$(g) with equilibrium constant $K_p$ at a particular temperature and pressure $P$. The degree of dissociation ($\alpha$) for PCl$_5$(g) is
Observe the following equilibrium in a 1 L flask:
A(g) <=> B(g)

At temperature T (in K), the equilibrium concentrations of A and B are 0.5 M and 0.375 M respectively.
Then 0.1 moles of A is added into the flask and the system is heated to temperature T again to re-establish equilibrium.

The new equilibrium concentrations (in M) of A and B respectively are:
$X_2(g) + Y_2(g) \rightleftharpoons 2Z(g)$. Equilibrium moles of $X_2, Y_2, Z$ are 3, 3, 9 mol (in 1 L). 10 mol of Z(g) is added. New equilibrium moles of Z(g) is ___. (Nearest integer)
For the reaction: \[ N_2O_3(g) \rightarrow NO(g) + NO_2(g) \] If the degree of dissociation is $\alpha = 0.2$, find $\Delta n_g$ and total number of moles at equilibrium (starting with 1 mole).
For the reaction \( \mathrm{A \rightleftharpoons B} \), the number of moles of A and B at equilibrium in a \(1\,\text{L}\) vessel are \(0.50\) and \(0.375\), respectively. If \(0.10\) mol of A is added further, determine the number of moles of A and B at the new equilibrium.
Consider the following electromagnetic waves A, B and C: (i) The wavelength of A is \(400\,\text{nm}\).
(ii) The frequency of B is \(10^{16}\,\text{s}^{-1}\).
(iii) Wave number of C is \(10^{4}\,\text{cm}^{-1}\).
The correct order of energies is:
Two moles each of the gases P$_2$, Q$_2$ and PQ are present in a vessel at equilibrium. If 1 mole each of P$_2$ and Q$_2$ is added at equilibrium, then determine the composition (in mole) of each species at the new equilibrium.
For a given reaction, K$_p$ = 9 atm
NH$_3$(g) $\longrightarrow$ $\frac{1}{2}$ N$_2$(g) + $\frac{3}{2}$ H$_2$(g)
Total pressure at equilibrium is $\sqrt{5}$ atm.
Find the value of 7$\alpha^2$, where $\alpha$ is degree of dissociation of NH$_3$(g)
For given reaction $X_2(g) + Y_2(g) \rightleftharpoons 2Z (g)$. Moles of $X_2, Y_2 & Z$ are at equilibrium are $3 \text{ mole}, 3 \text{ mole} & 9 \text{ mole}$ respectively. If $10 \text{ moles}$ of $Z$ are added at constant $T$ then find moles of $Z$ at re-established equilibrium.
The following concentrations were obtained in the formation of $NH_{3(g)}$ from $N_{2(g)}$ and $H_{2(g)}$ at equilibrium at $500\ \text{K}$: $[NH_{3}]=1.5\times10^{-2}\ \text{M}$, $[N_{2}]=5\times10^{-3}\ \text{M}$ and $[H_{2}]=0.10\ \text{M}$. Calculate the equilibrium constant $K_{c}$ for the reaction $N_{2(g)}+3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$.
For a reaction, \( A + B \rightleftharpoons 2C \), \( 1.0 \) mole of \( A \), \( 1.5 \) mole of \( B \) and \( 0.5 \) mole of \( C \) were taken in a \( 1\,L \) vessel. At equilibrium, the concentration of \( C \) was \( 1.0\,\text{mol L}^{-1} \). The equilibrium constant for the reaction is \( x/15 \). The value of \( x \) is:
At $27^\circ C$, the $K_a$ of acetic acid is $1.8 \times 10^{-5}$. What is the percentage of ionization of 0.02M of this acid at $27^\circ C$?

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:

In the following system, $ PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g) $ at equilibrium, upon addition of xenon gas at constant T and p, the concentration of
Given below are two statements:
Statement I: A catalyst cannot alter the equilibrium constant ($ K_c $) of the reaction, temperature remaining constant.
Statement II: A homogeneous catalyst can change the equilibrium composition of a system, temperature remaining constant.
In the light of the above statements, choose the correct answer from the options given below.

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]