Equilibrium CBSE Questions & Answers

Consider the following gaseous equilibria with equilibrium constants \({{\text{K}}_{\text{1}}}\) and \({{\text{K}}_{\text{2}}}\) respectively. \({\text{S}}{{\text{O}}_{{\text{2}}({\text{g}})}} + \frac{1}{2}{{\text{O}}_{{\text{2}}({\text{g}})}}\) \(\rightleftharpoons \) \({\text{S}}{{\text{O}}_{{\text{3}}({\text{g}})}}\)\({\text{2S}}{{\text{O}}_{{\text{3}}({\text{g}})}}\)\(\rightleftharpoons \)\({\text{2S}}{{\text{O}}_{{\text{2}}({\text{g}})}} + {\text{ }}{{\text{O}}_{{\text{2}}({\text{g}})}}\)The equilibrium constants are related as ______.

0.023 g of sodium metal is reacted with \({\text{1}}00{\text{ c}}{{\text{m}}^{\text{3}}}\) of water. The pH of the resulting solution is ______.

pH value of which one of the following is NOT equal to one?

\({{\text{H}}_{\text{2}}}{\text{S}}\) is passed into one \({\text{d}}{{\text{m}}^{\text{3}}}\) of a solution containing 0.1 mole of \({\text{Z}}{{\text{n}}^{{\text{2}} + }}\) and 0.01 mole of Cu2+ till the sulphide ion concentration reaches \({\text{8}}.{\text{1 }} \times {\text{ 1}}{0^{--{\text{19}}}}\) moles. Which one of the following statements is true? \(\left[ {{{\text{K}}_{{\text{sp}}}}{\text{of ZnS and CuS are 3 }} \times {\text{ 1}}{0^{--{\text{22}}}}{\text{and 8 }} \times {\text{ 1}}{0^{--{\text{36}}}}{\text{respectively}}} \right]\)

A vessel at 1000 K contains \({\text{C}}{{\text{O}}_{\text{2}}}\) with a pressure of 0.5 atm. Some of the \({\text{C}}{{\text{O}}_{\text{2}}}\) is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of K is

What is the best description of the change that occurs when \({\text{N}}{{\text{a}}_{\text{2}}}{\text{O}}\left( {\text{s}} \right)\) is dissolved in water?

Conjugate acid of a weak base is always stronger. What will be the decreasing order of basic strength of the following conjugate bases? \({\text{O}}{{\text{H}}^ - }\) , \(R{{\text{O}}^ - }\) , \({\text{CH3CO}}{{\text{O}}^ - }\), \({\text{C}}{{\text{l}}^ - }\)

Arrange the following in increasing order of pH \({\text{KN}}{{\text{O}}_{\text{3}}}\left( {{\text{aq}}} \right),{\text{C}}{{\text{H}}_{\text{3}}}{\text{COONa}}\left( {{\text{aq}}} \right),{\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl}}\left( {{\text{aq}}} \right),{{\text{C}}_{\text{6}}}{{\text{H}}_{\text{5}}}{\text{COON}}{{\text{H}}_{\text{4}}}\left( {{\text{aq}}} \right)\)

pH of a solution of a strong acid is 5.0. What will be the pH of the solution obtained after diluting the given solution a 100 times?

Following data is given for the reaction: \({\text{CaC}}{{\text{O}}_{\text{3}}}\left( {\text{s}} \right){\text{ }} \to {\text{ CaO }}\left( {\text{s}} \right){\text{ }} + {\text{ C}}{{\text{O}}_{\text{2}}}\left( {\text{g}} \right)\) \({\Delta _{\text{f}}}{\text{HV }}\left[ {{\text{CaO}}\left( {\text{s}} \right)} \right]{\text{ }} = {\text{ }}--{\text{ 635}}.{\text{1 kJ1mo}}{{\text{l}}^{--{\text{1}}}}\) \({\Delta _{\text{f}}}{\text{HV }}\left[ {{\text{C}}{{\text{O}}_{\text{2}}}\left( {\text{g}} \right)} \right]{\text{ }} = {\text{ }}--{\text{ 393}}.{\text{5 kJmo}}{{\text{l}}^{--{\text{1}}}}\) \({\Delta _{\text{f}}}{\text{HV }}\left[ {{\text{CaC}}{{\text{O}}_{\text{3}}}\left( {\text{s}} \right)} \right]{\text{ }} = {\text{ }}--{\text{ 12}}0{\text{6}}.{\text{9 kJmo}}{{\text{l}}^{--{\text{1}}}}\)Predict the effect of temperature on the equilibrium constant of the above Reaction (Hint: Apply Le-Chatelier’s principle)

Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume? \({\text{PC}}{{\text{l}}_{\text{5}}}\left( {\text{g}} \right)\) \( \rightleftharpoons \) \({\text{PC}}{{\text{l}}_{\text{3}}}\left( {\text{g}} \right){\text{ }} + {\text{ C}}{{\text{l}}_{\text{2}}}\left( {\text{g}} \right)\)

One of the reaction that takes place in producing steel from iron ore is the reduction of ironB. oxide by carbon monoxide to give iron metal and \({\text{C}}{{\text{O}}_{\text{2}}}\). \({\text{FeO }}\left( {\text{s}} \right){\text{ }} + {\text{ CO }}\left( {\text{g}} \right)!{\text{Fe }}\left( {\text{s}} \right){\text{ }} + {\text{ C}}{{\text{O}}_{\text{2}}}\left( {\text{g}} \right);{\text{Kp}} = {\text{ }}0.{\text{265 atm at 1}}0{\text{5}}0{\text{K}}\) What are the equilibrium partial pressures of CO and \({\text{C}}{{\text{O}}_{\text{2}}}\) at 1050 K if the initial partial pressures are: \({P_{co}}\)= 1.4 atm and \({P_{co2}}\) = 0.80 atm?

The ionization constant of HF is\({\text{3}}.{\text{2 x1}}{0^{ - {\text{4}}}}\).Calculate the degree of dissociation of HF in its 0.02 M solution. Calculate the concentration of all species present \((H3O + ,,{F^ - }andHF)\) in the solution and its H

Amines behave as

Assuming complete dissociation, calculate the pH of 0.002 M KOH solution.