TS EAMCET 18-July-2022 Shift 1 Solved Paper

For the reaction at equilibrium,
‌A(s)‌

⇌

=

B(s)+C(g)
‌K=‌

[B][C]

[A]

The concentrations of pure solids, pure liquids, and solvents are omitted from equilibrium constant expressions because they do not change significantly during reactions when enough amount is present to reach equilibrium. Therefore, the expression is written as, KC=[C]
Kp=pC(g), where pC(g) is the partial pressure of C. ∆H is dependent on temperature, if the reaction is exothermic, and the temperature is increased, the reaction enthalpy becomes more negative (more heat energy is released). If the reaction is endothermic, and the temperature is increased, the reaction enthalpy becomes more positive (more heat energy is absorbed).
∆H is independent of catalyst addition. The catalyst only decreases the activation energy of a reaction, thereby increases the reaction rate but does not affect the enthalpy of reaction.
So, statements (A), (B) and (D) are only correct.