For the reaction Ca(OH)2(aq) + 2HCl(aq) → CaCl2 (8) + 2H2O(1) AH° -30.2 kJ and AS° = 206 J/K The equilibrium constant for this reaction at 280.0 Kis Assume that AH° and As are independent of temperature.

Consider the reaction 2 NO₂(g) → N₂O4(9). (a) Using AGF N₂O4(g) = 97.79 kJ/mol and AGF NO₂(g) = 51.3 kJ/mol, calculate AGº at 298 K. -4.81 kJ (b) Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.30 atm and 1.35 atm, respectively. 4467.83 X KJ

Take all the thermodynamic data from your textbook. Assume the data do not vary with temperature. (a) Calculate AS uniy for the reaction H₂O₂(1)→ H₂O₂(g) at 178.0°C. Enter your answer in the box provided. J/K mol (b) Is the reaction spontaneous, nonspontaneous, or an equilibrium process? Select the best single answer. spontaneous O nonspontaneous an equilibrium process (c) The reaction NH3(g) + HCl(g) → NH4Cl(s) is spontaneous in the forward direction at room temperature. Determine the temperature at which it is no longer spontaneous in the forward direction. Enter your answer in the box provided. °C (d) Determine the boiling point of Br₂. Enter your answer in the box provided. °C

Consider the following reaction and the following conditions: Fe₂O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) AG = -2.8 x 104 J P(CO) = 1.4 atm, P(CO₂) = 2.1 atm (R = 8.314 J/mol-K) 1. The value for the Q is [Select] 2. The AG for the reaction at 298 K under the conditions shown is [Select]

Given the information A+ B → 2 D AH° = -776.1 kJ AS = 353.0 J/K С — D AH° = 493.0 kJ AS° = -222.0 J/K calculate AG at 298 K for the reaction А + В — 2С AG° = kJ

6C(s) + 6H₂(g) + 30₂(g) → CH₁₂O6 (s) 2Al(s) + Fe₂O₂ (s) → ALO₂ (s) + 2Fe(s) AH = - 1237. kJ AS = -3280. AG = kJ Which is spontaneous? this reaction O the reverse reaction neither AH = -852. kJ AS = J K J K AG 19. kJ Which is spontaneous? this reaction the reverse reaction neither

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For the reaction 2co(g) + O2(g)–→2CO2(g) AG° = -508.0 kJ and AS° = -173.1 JK at 335 K and 1 atm. The maximum amount of work that could be done by this reaction when 1.76 moles of CO(g) react at standard conditions at this temperature is kJ.

For a particular reaction at 199.1 °C, AG = -159.63 kJ, and AS = 894.41 J/K. Calculate AG for this reaction at 13.8 °C. AG = kJ

Consider the following reaction: H₂(g) + 12 (g) --> 2HI (g) Given the following data: H₂: AH° = 0 kJ/mol; Sº = 130 J/molk 12: AH°= 0 kJ/mol; Sº = 108 J/mol K HI: AH° = 26 kJ/mol; Sº = 201 J/mol K Determine the AGO in kJ for this reaction at 298K. Do not put units in your answer. Report your answer with two places past the decimal point.