Consider the following system at equilibrium where delta H degree = -108 kJ, and

Question

Consider the following system at equilibrium where delta H degree = -108 kJ, and K_c = 77.5. at 600 K CO(g) + Cl_2(g) COCl_2(g) If the TEMPERATURE on the equilibrium system is suddenly increased The value of K_c A. Increases B. Decreases C. Remains the same The value of Q_c A. Is greater than K_c B. Is equal to K_c c Is less than K_c 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 Cl_2 will: A. Increase B. Decrease C, Remain the same

Explanation / Answer

In an exothermic reaction, a decrease in temperature favours the reaction to occur in the forward direction

ans (A) Kc increases........Decrease T, ln K increases and therefore K increases, (because concentration of CH4 and CCl4 will increase whereas the concentration of CH2Cl2 will decrease

ans (C) and now since K is increased it will be greater than Q( Qc<Kc)

ans (A) Run in forward direction to restablish the equillibrium

ans (A) Incease

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