Chemical Equilibrium and its Characteristics

Which one of the following is NOT an example of heterogeneous equilibrium?

For the reaction ${\mathrm{Na}}_2{\mathrm{SO}}_4\left(\mathrm{s}\right)\rightleftharpoons 2{\mathrm{Na}}_{\text{(aq) }}{}^{+}+{{\mathrm{SO}}_4}^{2-}$ (aq) if $\mathrm{\Delta G}°=+58.7 \mathrm{kJ}$$,$ then find the value of ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{Na}}_2{\mathrm{SO}}_4$ in water at $27°\mathrm{C}$$.$

For the equilibrium, ${\mathrm{PCl}}_{5\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}$ at $298\mathrm{K},{\mathrm{K}}_{\mathrm{c}}=1.8\times {10}^{-7}$$.$ Then, $\mathrm{\Delta G}$for this reaction will be ______$[$Given $\log 4.5=0.6484$$]$

When reaction is carried out at standard states then at the equilibrium $\_\_\_\_\_\_\_\_\_\_$

$2S{\mathrm{O}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}\leftrightharpoons 2\mathrm{S}{\mathrm{O}}_{3\left(\mathrm{g}\right)}$

It is an example of _____ (homogeneous/ heterogeneous) equilibrium?

Which of the following is an example of homogeneous equilibrium?

Among the following, the correct statement about the chemical equilibrium is.

Which of the following statements is correct?

Which of the following graph will show the equilibrium condition for the reaction $\mathrm{A}\rightleftharpoons \mathrm{B}$ ?

Consider the reaction: $2 {\mathrm{N}}_2{\mathrm{O}}_{4 \left(\mathrm{g}\right)}\rightleftharpoons 4{\mathrm{NO}}_{2 \left(\mathrm{g}\right)}$ 

If $\frac{-\mathrm{d}\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]}{\mathrm{dt}}=\mathrm{K}{\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]}^1$

$\frac{+\mathrm{d}\left[{\mathrm{NO}}_2\right]}{\mathrm{dt}}={\mathrm{K}}^1{\left[ {\mathrm{N}}_2{\mathrm{O}}_4\right]}^1$ then correct relation is :-

When $1$ mole of ${\mathrm{N}}_2$ and $1$ mole of ${\mathrm{H}}_2$ is enclosed in $5 \mathrm{L}$ vessel and the reaction is allowed to attain equilibrium, it is found that at equilibrium there is $\mathrm{x}$ mole of ${\mathrm{H}}_2$. The number of moles of ${\mathrm{NH}}_3$ formed would be:

Which of the following statements is correct about establishment of equilibrium?

For the gaseous reaction $\mathrm{P}\mathrm{C}{\mathrm{l}}_5\left(\mathrm{g}\right)\rightleftharpoons \mathrm{P}\mathrm{C}{\mathrm{l}}_3\left(\mathrm{g}\right)+\mathrm{C}{\mathrm{l}}_2\left(\mathrm{g}\right)$, The degree of dissociation of  ${\mathrm{PCl}}_5$ is $50\%$ at $400 \mathrm{K}$ and $1.0 \mathrm{atm}$ pressure. Assuming ideal behaviour the density of equilibrium gaseous mixture will be:

Which of the following is a reversible reaction ?

In which direction does the reaction tend to shift to reach equilibrium given at a particular time, the analysis shows that composition of reaction mixture is 3.0 mol L^-1 N₂, 2.0 mol L^-1 H₂ and 0.5 mol L^-1 NH₃.

Equilibrium constant, K_c for the below reaction is

${\text{N}}_2\left(\text{g}\right)+{\text{3H}}_2\left(\text{g}\right)\rightleftharpoons {\text{2NH}}_3\left(\text{g}\right)\text{at 500 K is 0.061}$

 

$\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+2\mathrm{D}.....\left(\mathrm{i}\right)$

$\mathrm{A}+\mathrm{E}\rightleftharpoons \mathrm{C}+\mathrm{F}\dots \dots \dots .\left(\text{ii}\right)$

If ${\mathrm{K}}_1$ and ${\mathrm{K}}_2$ are equilibrium constants for the reactions $\left(\mathrm{i}\right)$ and $\left(\mathrm{ii}\right)$, respectively, then find out the equilibrium constant for the reaction $\mathrm{E}+2\mathrm{D}\rightleftharpoons \mathrm{B}+\mathrm{F}$.

Find the total pressure of cases over a mixture of X and Y, ​​​​​​​​when two solid compounds 'X' and 'Y' dissociates at a certain temperature is as follows:
$\mathrm{X}\left(\mathrm{s}\right)\rightleftharpoons \mathrm{A}\left(\mathrm{g}\right)+2\mathrm{B}\left(\mathrm{g}\right){\mathrm{Kp}}_1=9\times {10}^{-3}{\mathrm{atm}}^3$

$\mathrm{Y}\left(\mathrm{s}\right)\leftrightharpoons 2\mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right) {\mathrm{Kp}}_2=4.5\times {10}^{-3} {\mathrm{atm}}^3$

Calculate variation of EMF of a cell E, with temperature T, If $∆\mathrm{G}=∆\mathrm{H}-\mathrm{T}∆\mathrm{S}$ and $∆\mathrm{G}=∆\mathrm{H}+\mathrm{T}{\left[\frac{\mathrm{d}\left(∆\mathrm{G}\right)}{\mathrm{d}\mathrm{T}}\right]}_{\mathrm{p}}$.

Find the value of the equilibrium constant of the reaction $\text{x+y⇌z}$ at $227^{\circ }\text{C}$ whose $∆{\mathrm{G}}^{°}$ is equal to $-4.606 \mathrm{kcal}$.