[Review Topics] [References] Use the References to access important values if needed for this question. The free energy change for the following reaction at 25 °C, when [Co2+] = 1.14 M and [Cr*] = 8.46×10-³ M, is -279 kJ: 3C02*(1.14 M) + 2Cr(s)3Co(s) + 2Cr**(8.46x103 M) AG = -279 kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction? 9 more group attempts remaining Submit Answer Retry Entire Group

99+ [References] Use the References to access important values if needed for this question. Consider the reaction H₂(g) + Cl₂(g) →→→→2HCI(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of HCI(g) is reduced to 13.25 mm Hg, while the pressures of H₂(g) and Cl₂(g) remain at 1 atm. ANSWER: Submit Answer B kJ/mol Try Another Version 1 item attempt remaining Previous Next 3:18 AM 11/22/2022

The following reaction is exothermic. MgO(s) → Mg²+(g) + O2-(g) + 02 (g) O True False

What is the standard free energy change for the ionization of H2O2 acid, if its Ka is 2.40e-12.   66.326 kJ   -66.326 kJ   -152.749 kJ   152.749 kJ

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Consider the reaction 12(g) + Cl₂(g) 2ICI(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of ICI(g) is reduced to 16.66 mm Hg, while the pressures of l2(g) and Cl₂(g) remain at 1 atm. kJ/mol ANSWER: (Please type answer).

For the reaction CH4 (9) + H₂O(g) → 3H₂(g) + CO(g) AH = 206.1 kJ and AS = 214.7 J/K The standard free energy change for the reaction of 1.83 moles of CH4 (9) at 345 K, 1 atm would be kj. This reaction is favored under standard conditions at 345 K. Assume that AH and AS are independent of temperature.

For the reaction CO(g) + 3H₂(g) → CH4 (9) + H₂O(g) ΔΗ° - 206.1 kJ and AS = - 214.7 J/K The standard free energy change for the reaction of 1.67 moles of CO(g) at 253 K, 1 atm would be This reaction is favored under standard conditions at 253 K. Assume that AH° and AS° are independent of temperature. == kJ.

Calculate AG° and K, at 25 °C for the reaction 2 CO(g) + O2(g)→2 CO2(g) Is the reaction product-favored or reactant-favored under standard conditions? Thermodynamic Data: G'r (kJ/mol) Species CO(g) CO2(g) -137.17 -394.36 AG° = kJ/mol K, = O product-favored O reactant-favored