Please explain and provide answer Consider the following system at equilibrium w

Question

Please explain and provide answer

Consider the following system at equilibrium where H -108 k, and K.-775 , at 600 K: CO (g)+ Clh (g)CoCl2 (g) If the TEMPERATURE on the equilibrium system is suddenly increased The value of KeA. Increases B. Decreases C. Remains the same The value of QcA. 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 restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Cl2 will:A. Increase. B. Decrease C. Remain the same.

Explanation / Answer

Forward reaction is exothermic in nature

we are increasing temperature or adding heat here

so, according to Le Chatelier's principle,

equilibrium will move in direction which absorbs heat

hence, backward reaction will be favoured

Equilibrium moves to reactant side

So, value of Kc decreases

And Qc will become greater than Kc

It has to run in backward direction

The concentration of Cl2 will decrease

Answer:

B

A

B

A

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---