Equilibrium in Chemical Processes

Predict the extent of a reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)$ at $298 \mathrm{K}$ has $\mathrm{Kc}=4.8\times {10}^{-31}$.

${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right); \mathrm{Kc}=5.7\times {10}^{-9}$ at $298 \mathrm{K}$. At equilibrium

If $\mathrm{Kc}$ is very large 

Explain the classification of chemical equilibrium based on the extent of completion.

Equilibrium constant for the reaction, ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$ is $\mathrm{K}$, then equilibrium constant for the reaction, ${\mathrm{NH}}_3\rightleftharpoons \frac{1}{2}{\mathrm{N}}_2+\frac{3}{2}{\mathrm{H}}_2$ will be _____.

$\mathrm{A}:\sqrt{1/\mathrm{K}} \mathrm{B}:\sqrt{\mathrm{K}} \mathrm{C}:\sqrt{1/{\mathrm{K}}^2}$ (Enter your correct answer as $\mathrm{A}, \mathrm{B} \mathrm{or} \mathrm{C}$)

Classify equilibrium on the basis of physical state of its components. 

Identify the following reaction as homogeneous or heterogeneous equilibrium:

$2\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2\left(\mathrm{s}\right)\stackrel{ }{\rightleftharpoons }2\mathrm{PbO}\left(\mathrm{s}\right)+4{\mathrm{NO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$

Explain the classification of chemical equilibrium on the basis of extent of completion.

Which of the following statements is correct?

In terms of rate constants for forward and backward reactions (${\mathrm{k}}_{\mathrm{f}} \mathrm{and} {\mathrm{k}}_{\mathrm{b}}$), equilibrium constant of a reaction is equal to _____.

(A) $\frac{{\mathrm{k}}_{\mathrm{f}}}{{\mathrm{k}}_{\mathrm{b}}}$

(B) $\frac{{\mathrm{k}}_{\mathrm{b}}}{{\mathrm{k}}_{\mathrm{f}}}$

(C) $\frac{\mathrm{K}}{\mathrm{C}}$

Enter the correct answer as A, B or C.

Cotyledons are also called-

Which of the following is not a characteristic property of chemical equilibrium?

Which among the following is incorrect about equilibrium state?

The enthalpy and entropy change for the reaction are $30 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $105 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$, respectively. The temperature at which the reaction will be in equilibrium is

${\mathrm{Br}}_2 \left(\mathrm{l}\right)+{\mathrm{Cl}}_2 \left(\mathrm{g}\right)⟶2\mathrm{BrCl} \left(\mathrm{g}\right)$

Nitric oxide reacts with ${\mathrm{Br}}_2$ and gives nitrosyl bromide as per the reaction given below.

                      $2\mathrm{NO}\left(\mathrm{g}\right) + {\mathrm{Br}}_2\left(\mathrm{g}\right) \rightleftharpoons 2\mathrm{NOBr}\left(\mathrm{g}\right)$

When $0.087$ mole of $\mathrm{NO}$ and $0.0437$ mole of ${\mathrm{Br}}_2$ are mixed in a closed container at a constant temperature, $0.0518$ mole of $\mathrm{NOBr}$ is obtained at equilibrium. Calculate the equilibrium amount of $\mathrm{NO}$ and ${\mathrm{Br}}_2$.

Which are correct for a reversible reaction?

Based upon the following hypothetical equilibria at $273 \mathrm{K}$:

${\text{XCl}}_2·6{\text{H}}_2{\text{O}}_{\left(\text{s}\right)}\rightleftharpoons {\text{XCl}}_2·2{\text{H}}_2{\text{O}}_{\left(\text{S}\right)}+4{\text{H}}_2{\text{O}}_{\left(\text{v}\right)}{\text{ ; K}}_{\text{p}}{\text{ = 8.1 × 10}}^{\text{-11}}{\text{ atm}}^{\text{4}}$

${\text{Y}}_2{\text{HPO}}_4·12{\text{H}}_2{\text{O}}_{\left(\text{s}\right)}\rightleftharpoons {\text{Y}}_2{\text{HPO}}_4·7{\text{H}}_2{\text{O}}_{\left(\text{v}\right)}+5{\text{H}}_2{\text{O}}_{\left(\text{g}\right)}{\text{ ; K}}_{\text{p}}{\text{ = 3.2 × 10}}^{\text{-9}}{\text{ atm}}^{\text{5}}$

${\text{Z}}_2{\text{SO}}_4·10{\text{H}}_2{\text{O}}_{\left(\text{s}\right)}\rightleftharpoons {\text{Z}}_2{\text{SO}}_{4\left(\text{s}\right)}+10{\text{H}}_2{\text{O}}_{\left(\text{v}\right)}{\text{ ; K}}_{\text{p}}{\text{ = 1.0 × 10}}^{\text{-30}}{\text{ atm}}^{\text{10}}$

Which is the most effective dehydrating agent at $273 \mathrm{K}$? (Aqueous tension at $273 \mathrm{K}$ is $6.0 \times {10}^{-3}$ atm)

The equilibrium constant for the reaction,

${\text{N}}_{2\left(\text{g}\right)}+{\text{O}}_{2\left(\text{g}\right)}\rightleftharpoons 2{\text{NO}}_{\left(\text{g} \right)}$ at temperature $\mathrm{T}$ is  $4\times 10^{-4}$ . The value of ${\mathrm{K}}_{\mathrm{c}}$ for the reaction :

${\mathrm{NO}}_{\left(\mathrm{g}\right)}\leftrightharpoons \frac{1}{2}{\mathrm{N}}_{2\left(\mathrm{g}\right)} + \frac{1}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}$ at the same temperature is: