Consider the following reaction where Kp = 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) If...

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Chemistry

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.
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2.
Consider the following reaction where Kp = 2.74 at 1150K.Â 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.

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3.9 Ratings (360 Votes)

To answer questions we need to calculate Q value for bothreactionsGiven reaction is CO g Cl 2g COCl2 gThe K p value of reaction is K p P COCl 2 PCO x P Cl 2 157Q value of reaction P COCl 2 P CO x P Cl2 1 1 x 1 1Q K p reaction will proceed in forward direction1 Reaction will occur in which COCl 2 isproducedANSWER TRUE Q K pso reaction will proceed in forward direction to produce COCl2 2 K p will See Answer

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