Question

Thermochemistry question

Answer 1

Propene, C3H6(g) (molar mass 237.4g/mol), can be prepared by the dehydration of propanol, C3H7OH(g) (molar mass 324.7g/mol), using a solid catalyst. A

setup for the lab synthesis is shown in the diagram above. The equation for the dehydration reaction is given below.

C3H7OH(g) ⇒ C3H6(g) + H2O ΔH°298= 81.4 kJ/mol rxn; ΔS°298=101.4J/(J mol rxn)

A student added a 1.51 g samole of C3H7OH(l) to a test tube using the setup shown above. The student heated the test tube gently with a Bunsen burner until all of the C3H7OH(l) evaporated and gas generation stopped. When the reaction stopped, the volume of collected gas was 0.0854 L at 0.822 atm and 305 K. (The vapor pressure of water at 305K is 35.7 torr.)

a) Calculate the number of moles of C3H6(g)
(i) That are actually produced in the experiment and measured in the gas collected tube and
(ii) That would be produced if the dehydration reaction went to completion

b) Calculate the percent yield of C3H6(g) in the experiment

Because the dehydration reaction is not observed to occur at 298 K, the student claims that the reaction has an equilibrium constant less than 1.00 at 298 K.

c) Use the thermodynamic data to calculate ΔG°298 for the reaction. Explain what this answer means.

Answer 2

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