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Consider the following reaction where Kp = 10.5 at 350 K. 2CH2Cl2(g) CH4(g) + CCl4(g) If...

Consider the following reaction where Kp = 10.5 at 350 K. 2CH2Cl2(g) CH4(g) + CCl4(g) If the three gases are mixed in a rigid container at 350 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 CH2Cl2(g) is produced. 2. Kp will increase. 3. A reaction will occur in which CH4 is consumed. 4. Qp is greater than Kp. 5. The reaction is at equilibrium. No further reaction will occur.

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