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This is one of our many quizzes on Le Chatelier's principle. Click on this to access more such competitive quizzes on Chemical Equilibrium.

Le Chatelier's principle Quiz 2

chemistry

 What will happen if the temperature is increased for the following reaction $ \\ {{H}_{2}}(g)+{{I}_{2}}(g)\rightleftarrows 2HI(g) \\  \Delta {{n}_{g}}=0,\text{ }\Delta H=+ve $

  Le Chatelier's principle or the equilibrium law states that when a dynamic equilibrium is disturbed, the equilibrium will be restored by shifting the position of the equilibrium in an opposite direction.

Since the equilibrium is endothermic, an increase in temperature will shift the equilibrium forward and the yield of the HI will increase.

 While conducting an experiment, neon gas is introduced in a vessel containing $N{{O}_{2}}$ gas and ${{N}_{2}}{{O}_{4}}$ gas at equilibrium. The rate of dimerization of $N{{O}_{2}}$ gas $2N{{O}_{2}}(g)\rightleftarrows {{N}_{2}}{{O}_{4}}(g) \\  \Delta H=-57.2kJ/mol$

 Since inert gases do not participate in the reaction, the equilibrium is undisturbed, and hence there is no change in the rate of dimerization of $N{{O}_{2}}$ gas.

 Consider the following reaction $ \\ CO(g)+3{{H}_{2}}(g)\rightleftarrows C{{H}_{4}}(g)+{{H}_{2}}O(g) \\ $ When this reaction mixture is transferred to a vessel of half the volume, the yield of methane gas will

 Upon an increase in pressure in a gas phase reaction, according to Le Chatelier's principle, the equilibrium will shift so that fewer number gas molecules are produced.

 When volume is halved, pressure is doubled. $ \\ $ So, equilibrium will shift to the right as the moles of the products are less than the moles of the reactants and the yield of methane gas will increase.

 Given below are enthalpy diagrams for a reaction $ \\ $ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/b7976b04-3dd2-4e7d-9f2a-89e1c970717e3699493030383890536.png"/> $ \\ $ When the temperature of this reaction is increased, the yield of the product formed will

 According to Le Chatelier's principle, the increase in temperature will shift the equilibrium towards the left in an exothermic reaction, and towards the right in an endothermic reaction.

 The graph depicts an endothermic reaction. So, the yield of products formed will increase.

  The concentration of ${{H}_{3}}{{O}^{+}}$ ions increases in the solution when acid is added to pure water.

 Upon addition of acid to pure water, the equilibrium is disturbed, and to restore the ion-product constant of liquid water $({{K}_{w}})$ to ${{10}^{-14}}$, the equilibrium shifts towards the left, according to Le Chatelier's principle, and the concentration of $O{{H}^{-}}$ ions decreases.