164025 4 moles of \(A\) are mixed with 4 moles of \(B\), when \(2 \mathrm{~mol}\) of \(C\) are formed at equilibrium, according to the reaction, \(A+B \rightleftharpoons C+D\). The equilibrium constant is:

164026 \(A B\) dissociates as \(2 A B(g) \rightleftharpoons 2 A(g)+B_2(g)\) When the initial pressure of \(A B\) is \(500 \mathrm{~mm}\), the total pressure becomes \(625 \mathrm{~mm}\) when the equilibrium is attained. Calculate \(K_P\) for the reaction assuming volume remains constant.

164027 A reaction in equilibrium is represented by the following equation -
\(2 \mathrm{~A}_{(\mathrm{s})}+3 \mathrm{~B}_{(\mathrm{g})} \rightleftharpoons 3 \mathrm{C}_{(\mathrm{g})}+\mathrm{D}_{(\mathrm{g})}+Q\) if the pressure on the system is reduced to half of its original value:

164028 Two systems \(\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})\) and \(\mathrm{COCl}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g})\) are simultaneously in equilibrium in a vessel at constant volume. If some \(\mathrm{CO}(\mathrm{g})\) is introduced in the vessel at constant volume, then at new equilibrium the concentration of:

164029 \(\mathrm{aA}+\mathrm{bB} \rightleftharpoons \mathrm{cC}+\mathrm{dD}\)
in above reaction low pressure and high temperature, conditions shift the equilibrium in backward direction so correct set:

164025 4 moles of \(A\) are mixed with 4 moles of \(B\), when \(2 \mathrm{~mol}\) of \(C\) are formed at equilibrium, according to the reaction, \(A+B \rightleftharpoons C+D\). The equilibrium constant is:

164026 \(A B\) dissociates as \(2 A B(g) \rightleftharpoons 2 A(g)+B_2(g)\) When the initial pressure of \(A B\) is \(500 \mathrm{~mm}\), the total pressure becomes \(625 \mathrm{~mm}\) when the equilibrium is attained. Calculate \(K_P\) for the reaction assuming volume remains constant.

164027 A reaction in equilibrium is represented by the following equation -
\(2 \mathrm{~A}_{(\mathrm{s})}+3 \mathrm{~B}_{(\mathrm{g})} \rightleftharpoons 3 \mathrm{C}_{(\mathrm{g})}+\mathrm{D}_{(\mathrm{g})}+Q\) if the pressure on the system is reduced to half of its original value:

164028 Two systems \(\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})\) and \(\mathrm{COCl}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g})\) are simultaneously in equilibrium in a vessel at constant volume. If some \(\mathrm{CO}(\mathrm{g})\) is introduced in the vessel at constant volume, then at new equilibrium the concentration of:

164029 \(\mathrm{aA}+\mathrm{bB} \rightleftharpoons \mathrm{cC}+\mathrm{dD}\)
in above reaction low pressure and high temperature, conditions shift the equilibrium in backward direction so correct set:

164025 4 moles of \(A\) are mixed with 4 moles of \(B\), when \(2 \mathrm{~mol}\) of \(C\) are formed at equilibrium, according to the reaction, \(A+B \rightleftharpoons C+D\). The equilibrium constant is:

164026 \(A B\) dissociates as \(2 A B(g) \rightleftharpoons 2 A(g)+B_2(g)\) When the initial pressure of \(A B\) is \(500 \mathrm{~mm}\), the total pressure becomes \(625 \mathrm{~mm}\) when the equilibrium is attained. Calculate \(K_P\) for the reaction assuming volume remains constant.

164027 A reaction in equilibrium is represented by the following equation -
\(2 \mathrm{~A}_{(\mathrm{s})}+3 \mathrm{~B}_{(\mathrm{g})} \rightleftharpoons 3 \mathrm{C}_{(\mathrm{g})}+\mathrm{D}_{(\mathrm{g})}+Q\) if the pressure on the system is reduced to half of its original value:

164028 Two systems \(\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})\) and \(\mathrm{COCl}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g})\) are simultaneously in equilibrium in a vessel at constant volume. If some \(\mathrm{CO}(\mathrm{g})\) is introduced in the vessel at constant volume, then at new equilibrium the concentration of:

164029 \(\mathrm{aA}+\mathrm{bB} \rightleftharpoons \mathrm{cC}+\mathrm{dD}\)
in above reaction low pressure and high temperature, conditions shift the equilibrium in backward direction so correct set:

164025 4 moles of \(A\) are mixed with 4 moles of \(B\), when \(2 \mathrm{~mol}\) of \(C\) are formed at equilibrium, according to the reaction, \(A+B \rightleftharpoons C+D\). The equilibrium constant is:

164026 \(A B\) dissociates as \(2 A B(g) \rightleftharpoons 2 A(g)+B_2(g)\) When the initial pressure of \(A B\) is \(500 \mathrm{~mm}\), the total pressure becomes \(625 \mathrm{~mm}\) when the equilibrium is attained. Calculate \(K_P\) for the reaction assuming volume remains constant.

164027 A reaction in equilibrium is represented by the following equation -
\(2 \mathrm{~A}_{(\mathrm{s})}+3 \mathrm{~B}_{(\mathrm{g})} \rightleftharpoons 3 \mathrm{C}_{(\mathrm{g})}+\mathrm{D}_{(\mathrm{g})}+Q\) if the pressure on the system is reduced to half of its original value:

164028 Two systems \(\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})\) and \(\mathrm{COCl}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g})\) are simultaneously in equilibrium in a vessel at constant volume. If some \(\mathrm{CO}(\mathrm{g})\) is introduced in the vessel at constant volume, then at new equilibrium the concentration of:

164029 \(\mathrm{aA}+\mathrm{bB} \rightleftharpoons \mathrm{cC}+\mathrm{dD}\)
in above reaction low pressure and high temperature, conditions shift the equilibrium in backward direction so correct set:

164025 4 moles of \(A\) are mixed with 4 moles of \(B\), when \(2 \mathrm{~mol}\) of \(C\) are formed at equilibrium, according to the reaction, \(A+B \rightleftharpoons C+D\). The equilibrium constant is:

164026 \(A B\) dissociates as \(2 A B(g) \rightleftharpoons 2 A(g)+B_2(g)\) When the initial pressure of \(A B\) is \(500 \mathrm{~mm}\), the total pressure becomes \(625 \mathrm{~mm}\) when the equilibrium is attained. Calculate \(K_P\) for the reaction assuming volume remains constant.

164027 A reaction in equilibrium is represented by the following equation -
\(2 \mathrm{~A}_{(\mathrm{s})}+3 \mathrm{~B}_{(\mathrm{g})} \rightleftharpoons 3 \mathrm{C}_{(\mathrm{g})}+\mathrm{D}_{(\mathrm{g})}+Q\) if the pressure on the system is reduced to half of its original value:

164028 Two systems \(\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})\) and \(\mathrm{COCl}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g})\) are simultaneously in equilibrium in a vessel at constant volume. If some \(\mathrm{CO}(\mathrm{g})\) is introduced in the vessel at constant volume, then at new equilibrium the concentration of:

164029 \(\mathrm{aA}+\mathrm{bB} \rightleftharpoons \mathrm{cC}+\mathrm{dD}\)
in above reaction low pressure and high temperature, conditions shift the equilibrium in backward direction so correct set: