Chemistry - Chemical Equilibrium Question with Solution | TestHub
How many statements regarding the following equilibrium are correct?
(i) On increasing P at constant T, state of equilibrium shifts in backward direction.
(ii) On decreasing V at constant T, state of equilibrium shifts in backward direction.
(iii) On increasing T, state of equilibrium shifts in backward direction.
(iv) On addition of 10 gm of B(s), state of equilibrium shifts in backward direction.
(v) On increasing T, equilibrium constant of the reaction decreases.
(vi) On increasing V at constant T equilibrium constant of the reaction decreases.
(vii) On increasing P at constant T, equilibrium constant of the reaction decreases.
(viii) On adding 10 gm of B(s) at constant T, equilibrium constant of the reaction decreases.
Answer:
Solution:
Reaction Properties: The reaction is exothermic () and increases gaseous moles ().
Pressure & Volume: Statements (i) and (ii) are correct because increasing pressure (or decreasing volume) shifts the equilibrium backward toward fewer gas moles.
Temperature Effect: Statements (iii) and (v) are correct because increasing temperature shifts an exothermic reaction backward and decreases its equilibrium constant ().
Incorrect Statements: Statements (iv), (vi), (vii), and (viii) are false because pure solids do not alter equilibrium, and depends solely on temperature.
Conclusion: The total number of correct statements is 4 [statements (i), (ii), (iii), and (v)].
