In the Haber process, ammonia is synthesized from N2 and H2: N2 (g) + 3 H, (g) 2 NH3 (g) AG° at 298 K for this reaction is –33.3 kJ/mol. The value of AG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2 and 0.65 atm NH; is kJ. а) —1.8 b) -3.86 х 103 NH3- c) -7.25 x 103 H2 -N2 d) -104.5 e) -40.5

In the Haber process, ammonia is synthesized from N2 and H2: N2 (g) + 3 H, (g) 2 NH3 (g) AG° at 298 K for this reaction is –33.3 kJ/mol. The value of AG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2 and 0.65 atm NH; is kJ. а) —1.8 b) -3.86 х 103 NH3- c) -7.25 x 103 H2 -N2 d) -104.5 e) -40.5

Chemistry

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Chapter17: Spontaneity, Entropy, And Free Energy

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Problem 70E: Hydrogen sulfide can be removed from natural gas by the reaction 2H2S(g)+SO2(g)3S(s)+2H2O(g)...

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At 298 K, G = 70.52 kJ for the reaction 2NO(g) + O2(g) 2NO2(g) (a) Calculate _G at the same temperature when PNO = 1.0 104 atm, PO2=2.0103 atm, and PNO2=0.30 atm. (b) Under the conditions in part a, in which direction is the reaction spontaneous?
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
One of the reactions that destroys ozone in the upper atmosphere is NO(g)+O3(g)NO2(g)+O2(g) Using data from Appendix 4, calculate G and K (at 298 K) for this reaction.
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the synthesis of ammonia? 3H2(g) + N2(g) 2NH3(g)
Explain why absolute entropies can be measured.
What types of experiments can be carried out to determine whether a reaction is spontaneous? Does spontaneity have any relationship to the final equilibrium position of a reaction? Explain.
Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?
Many biochemical reactions that occur in cells require relatively high concentrations of potassium ion (K+). The concentration of K + in muscle cells is about 0.l5 M. The concentration of K+ in blood plasma is about 0.0050 M. The high internal concentration in cells is maintained by pumping K+ from the plasma. How much work must be done to transport 1.0 mole of K+ from the blood to the inside of a muscle cell at 37C, normal body temperature? When 1.0 mole of K+ is transferred from blood to the cells, do any other ions have to be transported? Why or why not?
Use data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?
Chemists and engineers who design nuclear power plants have to worry about high-temperature reactions because it is possible for water to decompose. (a) Under what conditions does this reaction occur spontaneously? 2H2O(g) 2H2(g) + O2(g) (b) Under conditions where the decomposition of water is spontaneous, do nuclear engineers have to worry about an oxygen/hydrogen explosion? Justify your answer.
Hydrogen sulfide can be removed from natural gas by the reaction 2H2S(g)+SO2(g)3S(s)+2H2O(g) Calculate G and K (at 298 K) for this reaction. Would this reaction be favored at a high or low temperature?
On the basis of your experience, predict which of the following reactions are spontaneous. (a) CO2(s)CO2(g) at 25C (b) NaCl(s)NaCl(l) at 25C (c) 2NaCl(s)2Na(s)+Cl2(g)(d) CO2(g)C(s)+O2(g)

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