Practice ProblemATTEMPT
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CHEMISTRY(HARDCOVER W/CODE) CUSTOM
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- Calculate K at 298 K for the following reaction: NO(g) + 1/2 O2 (g) <-> NO2 (g) Delta G (kJ/mol) for the following: NO(g) 86.60, NO2(g) 51, O2(g) 0 (answer in scientific notation)arrow_forwardSolve all part please. Consider the equilibrium reaction N2O4 (g) ⇌ 2 NO2 (g)a. Using appendix C, find H and S for this reaction (you will need this for b,c). delta s= 176.6J delta H=5802kJb. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PNO2 = PN2O4 = 1.0 atm.c. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PT = 10.0 atm and PNO2 = 2 PN2O4.arrow_forwardThe standard free-energy change for the Haber process at 25 °C was obtained in Sample Exercise 19.9 for the Haber reaction:N21g2 + 3 H21g2 ∆ 2 NH31g2 ∆G° = -33.3 kJ>mol = -33,300 J>mol Use this value of ∆G° to calculate the equilibrium constant for the process at 25 °C.arrow_forward
- If the value of AG is less than zero, it indicates that the reaction is. A. Spontaneous B. reaction is at equilibrium C. nonspontaneous D. none from the choices.arrow_forwardIn what condition, a reaction is product-favored. Select the correct answer... a. K° = 0 and G° = 0. b. K° < 1 and G° = 0. c. K° < 1 and G° > 0. d. K° > 1 and G° < 0. e. K° = 1 and G° = 0.arrow_forwardPredict the sign of S and then calculate S for each of the following reactions. a. 2H2S (g) + SO2(g) 3Srhommbic(s) + 2H2O(g) b. 2SO3 (g) 2SO2(g) + O2(g) c. Fe2O3(s) + 3H2(g) 2Fe(s) + 3H2O (g)arrow_forward
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