please help me answer all these correctly. the second picture asks whether each
ID: 1028470 • Letter: P
Question
please help me answer all these correctly. the second picture asks whether each one increases, decreases, or remains the same or no change
Consider the following system at equilibrium where H -108 kJ, and K.-1.29x10", at 600 K: If the TEMPERATURE on the equilibrium system is suddenly decreased The value of KeA Increases B. Decreases C. Remains the same The value of Q.[ ] A. Is greater than Ke B. Is equal to Ke C. Is less than Ke The reaction must:A Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium C. Remain the same. Already at equilibrium. The concentration of Ch will: A. Increase. B. Decrease. C. Remain the same.Explanation / Answer
Since Delta H value is positive, the reaction is endothermic and occurs at high temperatures.
On decreasing the temperature the reaction moves in backward direction.
Hence Kc value decreases
Qc value increases and greater than Kc
Equilibrium shifts in reverse direction
2. A/c to Le Chatlier's principle, if we add any materials, the equilibrium always shifts in a direction to decrease the concentration of the added material. Hence here we are adding PCl5,to decrease the concentration of the PCl5 (by consuming) equilibrium shifts in forward direction.
Hence Kc value increases
Qc value decreases
Reaction moves in forward direction
And concentration of PCl3 and Cl2 increases
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