(a) 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 increase. 3. A reaction will occur in which CO is consumed. 4. Q is less than K. 5. The reaction is at equilibrium. No further reaction will occur. (b) Consider the following reaction where Kc = 34.5 at 1150 K: 2SO2(g) + O2(g) 2SO3(g) A reaction mixture was found to contain 4.37×10-2 moles of SO2(g), 3.96×10-2 moles of O2(g) and 3.91×10-2 moles of SO3(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium SO3(g) must be produced. 2. In order to reach equilibrium Kc must increase. 3. In order to reach equilibrium SO2 must be produced. 4. Qc is less than Kc. 5. The reaction is at equilibrium. No further reaction will occur.
(a) 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 increase.
3. A reaction will occur in which CO is consumed.
4. Q is less than K.
5. The reaction is at equilibrium. No further reaction will occur.
(b) Consider the following reaction where Kc = 34.5 at 1150 K:
2SO2(g) + O2(g) 2SO3(g)
A reaction mixture was found to contain 4.37×10-2 moles of SO2(g), 3.96×10-2 moles of O2(g) and 3.91×10-2 moles of SO3(g), in a 1.00 Liter container.
Indicate True (T) or False (F) for each of the following:
1. In order to reach equilibrium SO3(g) must be produced.
2. In order to reach equilibrium Kc must increase.
3. In order to reach equilibrium SO2 must be produced.
4. Qc is less than Kc.
5. The reaction is at equilibrium. No further reaction will occur.
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