chemistry homework help concerning vaporization, boiling point, ΔH, K,and heat?
The normal boiling point of pyridine is 115 °C. It turns out that ΔS of vaporization for most liquids is around 90 J/K. Which of the following statements is false?
1. At 110 °C the value of K for this reaction is less than 1.
2. At 120 °C the value of K for this reaction is greater than 1.
3. One mole of pyridine releases about 34.9 kJ/mol of heat when it condenses.
4.The value of ΔH of vaporization is around 34.9 kJ/mol
5. At 115 °C, the equilibrium constant for pyridine(l) to pyridine(g) is equal to zero
Please explain your logic behind the answer. I'm at a total loss. Thank you in advance!
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The answer is 5.
Why:
K is equal to 1 at the boiling point because the equation C5H5N(l)<->C5H5N(g) is at equilibrium between the two phases. K should be above 1 if it favors the products, in this case it favors the gas phase, (like in option 2), and it should be below 1 if it favors the reactants a.k.a. the liquid phase (like in option 1). If it is in equilibrium (the boiling point) and favors neither, it should be right at 1.
Options 3 and 4 you can calculate from the equation S=H/T (you know s is 90J and T is 298K at room temp) to convince yourself those are true. Note that in option 3 the it releases the energy because it is condensing not boiling.
Their Boiling elements. Throughout a separation system of two specific boiling point liquids, cautious temperature manipulate and commentary is required to be able to notice the ultimate Boiling factor (FBP) of the lighter liquid. This will be the preliminary Boiling point (IBP) of the following (heavier) liquid.