Consider the following reaction where Kp = 1.57 at 600 K: CO(g)+ Cl2(g) COCl2(g) If the three gases are mixed in a rigid containerat 600 K so that the partial pressure of each gas is initially oneatm, what will happen?
Indicate True (T) or False (F) for each of the following:
1. A reaction will occur in which COCl2(g) is produced
2. Kp will decrease.
3. A reaction will occur in which CO is produced.
4. Q is less than K
. 5. The reaction is at equilibrium. No further reaction willoccur.
--------------------------------------------------------------------------------------
2.
Consider the following reaction where Kp = 2.74 at 1150K. Â
2SO3(g) 2SO2(g) + O2(g)Â Â
If the three gases are mixed in a rigid container at 1150 K so thatthe partial pressure of each gas is initially one atm, what willhappen?
Indicate True (T) or False (F) for each of the following:
___
T
F
1. A reaction will occur in which SO3(g) is produced.
___
T
F
2. Kp will increase.
___
T
F
3. A reaction will occur in which SO2 is consumed.
___
T
F
4. Qp is greater than Kp.
___
T
F
5. The reaction is at equilibrium. No further reaction willoccur.
