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Question 1 of 3
1. Question
Pure N2O4(g) was added to an empty, closed flask at 127 °C until the pressure reached 4.38 × 10-2 atm. The system was allowed to come to equilibrium according to the following equation.
At equilibrium, the total pressure in the flask was 7.43 × 10-2 atm. What is the value of Kp for this reaction?
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Question 2 of 3
2. Question
A 2.50 mole quantity of NOCl was placed in an empty, 1.50 L rigid container at 400 °C. After equilibrium was established, it was found that 28.0% of the NOCl had dissociated according to the following equation.
Determine Kc for the reaction.
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Question 3 of 3
3. Question
Gaseous acetic acid, CH3CO2H, is in equilibrium with its gaseous dimer, (CH3CO2H)2, as shown below.
If the total pressure at equilibrium is 1.48 atm and Kp = 3.62, what is the partial pressure of the dimer?
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