List of top Chemistry Questions on Equilibrium asked in KCET

Given E⁰_Fe+3/Fe+2=+0.76V and E⁰½2l^-=+0.55V. The equilibrium constant for the reaction taking place in galvanic cell consisting of above two electrodes is [\(\frac{2.303RT}{F}\)=0.06]

Acidity of $BF_3$ can be explained on which of the following concepts ?

The relationship between $K_p$ and $K_c$ is $K_p=K_c (RT)^{\Delta n}$ What would be the value of $\Delta n$ for the reaction : $NH_4Cl_{(s)} <=> NH3_{(g)} +HCl_{(g)}$ ?

The equilibrium constant for the reaction $N _{2( g )}+ O _{2( g )} \rightleftharpoons 2 NO _{( g )}$ is $4 \times 10^{-4}$ at $2000\,K$. In presence of a catalyst the equilibrium is attained ten times faster. Therefore the equilibrium constant in presence of catalyst of $2000\, K$ is

The reaction quotient '$Q$' is useful in predicting the direction of the reaction. Which of the following is incorrect ?

Equilibrium constants $K_1$, and $K_2$ for the following equilibria I. $NO _{( g )}+\frac{1}{2} O _{2( g )} \rightleftharpoons NO _{2( g )}$ II. $2 NO _{2( g )} \rightleftharpoons 2 NO _{( g )}+ O _{2( g )}$ are related as :

In presence of $HCl, H_2S$ results the precipitation of Group-2 elements but not Gp-4 elements during qualitative analysis. It is due to

For the equilibrium : $CaCO_{3_(s)} \leftrightharpoons CaO_{(s)}+CO_{2(g)}$; $K_p = 1.64 \,atm \,at \,1000\, K$ $50\, g$ of $CaCO_3$ in a $10\, litre$ closed vessel is heated to $1000\, K$. Percentage of $CaCO_3$ that remains unreacted at equilibrium is (Given $R \,= \,0.082\, L \,atm \,K^{-1} mol^{-1}$)

An example for a neutral buffer is

$5\, ml$ of $0.4\, N\, NaOH$ is mixed with $20\, ml$ of $0.1\, N\, HCl$. The $pH$ of the resulting solution will be

On adding which of the following, the pH of $20\, ml$ of $0.1\, N\, HCl$ will not alter ?

Consider the following gaseous equilibria with equilibrium constants $K_1$ and $K_2$ respectively. $SO_{2(g)} + \frac{1}{2} O_{2(g)} \leftrightharpoons SO_{3(g)}$ $2SO_{3(g)} \leftrightharpoons 2SO_{2(g)} + O_{2(g)}$ The equilibrium constants are related as

For the reversible reaction $A_{(s)}+B_{(g)}\leftrightharpoons C_{(g)} +D_{(g)} \Delta G^\circ=-350kJ $ which one of the following statements is true?

$0.023\, g$ of sodium metal is reacted with $100 \,cm^3$ of water. The pH of the resulting solution is ______

For the reversible reaction $A_{(s)}+B_{(g)} \rightleftharpoons C_{(g)}+D_{(g)}: \Delta G^{0}=-350 kJ .$ Which one of the following statements is true?

$5$ moles of $SO_2$ and $5$ moles of $O_2$ are allowed to react. At equilibrium, it was found that $60\% $ of $SO_2$ is used up. If the partial pressure of the equilibrium mixture is one atmosphere, the partial pressure of $O_2$, is

$10^{-6}\, M\, NaOH$ is diluted $100$ times. The $pH$ of the diluted base is

$30\, cc$ of $\frac {M}{3}\, HCl, 20\, cc$ of $\frac {M}{N} HNO_3$ and $40\, cc$ of $\frac {M}{4}$ $NaOH$ solutions are mixed and the volume was made up to $1\, dm^3$. The $pH$ of the resulting solution is

Three moles of $PCl_5$, three moles of $PCl_3$ and two moles of $Cl_2$ are taken in a closed vessel. If at equilibrium the vessel has $1.5$ moles of $PCl_5$, the number of moles of $PCl_3$ present in it is

Hydroxyl ion concentration of $1M\, HCl$ is

$4$ moles each of $S O_{2}$ and $O_{2}$ gases are allowed to react to form $SO_{3}$ in a closed vessel. At equilibrium $25 \%$ of $O_{2}$ is used up. The total number of moles of all the gases present at equilibrium is

For the reaction $N_{2(s)}+O_{2(s)} \rightleftharpoons 2 N O_{(g)}$, the value of $K_{c}$ at $800^{\circ} C$ is $0.1 .$ When the equilibrium concentrations of both the reactants is $0.5 \,mol$, what is the value of $K_{P}$ at the same temperature?

A buffer solution has equal volumes of $0.2M \, NH_4OH$ and $0.02\, M \, NH_4 Cl$. The $p^{kb}$ of the base is $5$. The $pH$ is

$15 $ moles of $H_2$ and $5.2$ moles of $I_2$ are mixed and allowed to attain equilibrium at $500^\circ$C. At equilibrium, the concentration of $HI$ is found to be $10$ moles. The equilibrium constant for the formation of $HI$ is

In the manufacture of ammonia by the Haber's process, ${N_{2(g)} +3H_{2(g)} <=> 2NH_{3(g)} + 92.3 kJ} $, which of the following conditions is unfavourable ?