Problem_Set__10

# Problem_Set__10 - c Calculate the value of the equilibrium...

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Chemistry 2080 Spring 2009 Problem Set #10 - due date: Friday, April 24th at 2 pm Name:________________ Lab TA Name:__________________ Lab Day/Time:______________________ Practice problems (not graded). Chapter 19 : 7, 15, 17, 22, 23, 31, 35, 39, 53, 63 1) Iron(III) oxide can be reduced with carbon monoxide to make metallic iron. The carbon monoxide becomes oxidized to carbon dioxide: Fe 2 O 3 (s) + 3CO(g) –––––> 2Fe(s) + 3CO 2 (g) We have the following values of Δ f and S° for the four components of this reaction: Fe 2 O 3 (s) CO(g) Fe(s) CO 2 (g) Δ f {kJ/mol} -824.2 -110.5 0 -393.5 {J/(K.mol)} +87.40 +197.7 +27.28 213.7 a) Calculate the standard free-energy change for the above reaction at 25°C. b) Would the reaction as written be spontaneous under standard-state conditions at 25°C ?

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Unformatted text preview: c) Calculate the value of the equilibrium constant for the above reaction at 25°C. d) Would the reverse reaction become spontaneous at higher temperatures? 2) The Haber synthesis of ammonia from nitrogen and hydrogen is as follows: N 2 (g) + 3H 2 (g) –––––> 2NH 3 (g) (a) Using only the following data for ammonia ( Δ H° f = – 46.1 kJ/mol, and Δ G° f = – 16.5 kJ/mol); calculate Δ H° and Δ S° for the reaction at 25°C (b) Account for the sign of Δ S° (c) Is the reaction spontaneous under standard-state conditions at 25°C ? Explain. (d) What are the equilibrium constants K p and K c for the reaction at 350 K? (You may assume that Δ H° and Δ S° are both independent of temperature)....
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