Consider the following system at equilibrium where H-879 kJ, and Ke-1.20x10-2, a
ID: 569366 • Letter: C
Question
Consider the following system at equilibrium where H-879 kJ, and Ke-1.20x10-2, at 500 K. PCIs(g)PCl3(g) +C128 If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of Ke LJA. increases. B. decreases. C. remains the same. The value of Qe A. is greater than Kc B. is equal to Kc C. is less than Kc Ann in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The reaction must: A. increase. B. decrease. C. remain the same. The number of moles of Cl2 will:Explanation / Answer
PCl5(g) <- - - - - - - > PCl3(g) + Cl2(g)
Kc = [PCl3] [Cl2] /[PCl5]
In this reaction, no of moles is increased in product side
i) The value of Kc
C) remais the same
Equillibrium constant will not change by change in concentration
ii) The value of Qc
C) is less than Kc
As the no of moles increased in product side, while increasing the volume the equillibrium shift move to the product side, for this shift Qc<Kc.
iii) The reaction must
A) run in the forward direction to reestablish equillibrium.
iv) The no of moles of Cl2 will
A) increase