Consider the following reaction where Kp = 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g
ID: 1066940 • Letter: C
Question
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 container at 600 K so that the partial pressure of each gas is initially one atm, 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 will occur.
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2.
Consider the following reaction where Kp = 2.74 at 1150 K.
2SO3(g) 2SO2(g) + O2(g)
If the three gases are mixed in a rigid container at 1150 K so that the partial pressure of each gas is initially one atm, what will happen?
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 will occur.
Explanation / Answer
Qp = p(COCl2) /{pCO * pCl2}
= 1*1/1
=1
Qp < Kp so, reaction will move to right
1. A reaction will occur in which COCl2(g) is produced
True
2. Kp will decrease.
kp doesn't change. it depends on temperature only
False
3. A reaction will occur in which CO is produced.
False
4. Q is less than K
True
5. The reaction is at equilibrium. No further reaction will occur.
false
I am allowed to answer only 1 question at a time