Consider the following reaction: 2 NO(g)  N2(g) + O2(g) The enthalpy change at 298 K for this reaction is Horxn = -180.74 kJ/mol. Under the same conditions the entropy change for the reaction is Sorxn = -24.71 J/mol-K. Calculate the value of Keq for this reaction at 8214 K. Assume that Horxn

The following is known as the thermite reaction:2 Al(s) + Fe2O3(s)-----> Al2O3(s) + 2 Fe(s)This highly exothermic reaction is used for welding massiveunits, such as propellers for large ships. Using standard enthalpiesof formation in Appendix C, calculate ΔH ° for thisreaction.

Propylene glycol (C3H8O2) is an important compound used to de-ice airplanes before take-off and as RV antifreeze due to it being relatively non-toxic. A plausible reaction for the production of ethylene glycol is:  2 CO (g) + 2 H2 (g) + CH4 (g) -> C3H8O2 (l)  Using the thermodynamic properties from the following table, what is the value for ΔrS°, in units of J K-1‑mol-1 at 25 °C? Substance  ΔfH° (kJ/mol)  S° (J/Kmol)  CO (g)  -110.5  197.7  H2 (g)  0  130.7  CH4 (g)  -74.6  186.3  C3H8O2 (l)  -429.8  93.7

The standard enthalpy change and standard entropy change for the reaction are: A,Hº = -666.2 kJ mol-1 and A,S° = -114.0 J K-1 mol-1, respectively. Which of the following statements is true? O The reaction is non-spontaneous at all temperatures. The reaction is only spontaneous at high temperatures. The reaction spontaneous at all temperatures. O The reaction is spontaneous at low temperatures.

Consider the following reaction at 25 °C: 3 Ni(s) + N2(g) + 3 H2O(g) → 3 NiO(s) + 2 NH:(g) Given the information in the table, calculate AH° for the reaction. Compound AHº (kJ/mol) (J/mol·K) NiO (s) -239.7 38.0 Ni (s) 29.9 NH3 (g) -46.0 192.5 N2 (g) 191.5 H2O (g) -241.8 188.7

For the reaction 4HCI(g) + O2(g) 2H20(g) + 2Cl2(g) AH° = -114.4 kJ and AS° = -128.9 J/K The maximum amount of work that could be done when 1.95 moles of HCI(g) react at 311 K, 1 atm is kJ. Assume that AH° and AS° are independent of temperature.

For a particular reaction at 179.4 °C, AG = -801.20 kJ, and AS = 915.51 J/K. Calculate AG for this reaction at -52.5 °C. AG =

Consider a chemical reaction with a change in enthalpy of 845 kJ/mol and a change in entropy of 2,334 J/(mol·K). Heather believes this reaction is only thermodynamically favorable at high temperatures, but Everley believes this reaction is only thermodynamically favorable at low temperatures. Which student do you agree with, if either? Justify your response using the equation you would use to solve this problem

Use the data in the table to calculate the ΔH°rxn of the following reaction at 298 K:  HI(g) + ICl(g) --> HCl(g) + I2(g)         SPECIES       ΔH° at 298 (kJ/mol)        ------------------------------------------------------------------------------         HCl(g)            -92.31            I2(s)               0               I2(g)             62.44             ICl(g)             17.78           HI(g)              26.5

The reaction: 2 Mg + O2 --> 2 MgO has Δ Hrxn = -600. kJ/mol. Determine q for the reaction of 10.0 g of Mg according to the equation above.