Estimate the value of the equilibrium constant at 675 K for each of the following reactions. Part A 2 NO2(g) = N204(9) Standard Thermodynamic Quantities for Selected Substances at 25 °C Substance Af H° (kJ mol¯1) S° (J K-1 mol-) NO2(9) 33.2 240.1 N2O4(9) 9.16 304.4 ? K = Submit Request Answer

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Is the following chemical reaction spontaneous or non-spontaneous? 31 (aq) + H3ASO4(ag) + 2H* 3 (aq) + H3ASO3(aq) + H2O) (aq) Substance or ion AH°{(kJ/mole) S° (J/mole*K) -55.19 180.7 I (aq) H3ASO4(aq) -345.69 212.34 -11.23 11.09 H* (ag) 69.77 -89.6 13 (aq) H3ASO3(aq) -301.27 199.78 H20 (1) -285.8 69.95 the enthalpy must be calculated first both spontaneous and non-spontaneous

< ✓ 11 Question 25 of 25 (1 point) | Question Attempt: 1 of 2 ✓ 12 ✓ 13 ✓ 14 Here are some facts about the reaction: ✓ 15 At -5.67 °C the concentration equilibrium constant K = 7.0 for a certain reaction. с • If the reaction is run at constant pressure, 101. kJ/mol of heat are absorbed. X 16 -1 1 • The constant pressure molar heat capacity C₂ = 2.23 J-mol K Р Using these facts, can you calculate Kat 9.4 °C? • If the reaction is run at constant pressure, the volume increases by 13.%. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 9.4 °C will be bigger or smaller than Kat -5.67 °C? O Yes. O No. 0 17 Yes, and K will be bigger. No. Yes, and K will be smaller.