Consider the following system at equilibrium where H:198 ki, and Kc-345, at 1.15
ID: 1083362 • Letter: C
Question
Consider the following system at equilibrium where H:198 ki, and Kc-345, at 1.15x103 K: 2 so2 (g)-02 (g) 2 SO3 (g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value of KcA. Increases B. Decreases C. Remains the same The value ofQcA. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must:A Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to C. Remain the same. Already at equilibrium. The concentration of O2 will: A. Increase. B. Decrease. C. Remain the same.Explanation / Answer
A/C to Le Chatlier's principle, if we if we change concentration, volume, pressure and temperature then the equilibrium will shift in a direction to nullify that change.
Since the forward reaction is exothermic (Delta H is negative), increase in temperature is endothermic reaction and moves in backward direction.
1. Option B, Kc decrease in backward direction
2. Option A, Qc greater than Kc since reaction moves in backward direction
3. Option B, reverse direction
4. Option A, increases since reaction favors reverse direction.
Hint : Q> K - reaction moves to left
Q< K - reaction moves to right
Q=K, since equilibrium