A student determines the value of the equilibrium constant to be 8.18x10-37 for the following reaction. H₂S(g) + 2H₂O(l)—3H₂(g) + SO₂(g) Based on this value of Keq: AG° for this reaction is expected to be (greater, less) zero. than Calculate the free energy change for the reaction of 1.68 moles of H₂S(g) at standard conditions at 298K. AG rxn= kJ

At room temperature (25°C), the equilibrium constant (Kw) for the self-ionization of water is 1.00 × 10−14. Using this information, calculate the standard free energy change for the aqueous reaction of hydrogen ion with hydroxide ion to produce water at 25°C. (Hint: The reaction is the reverse of the self-ionization reaction.)

ΔG° for the reaction shown is equal to -419.6 (kJ/mol). Use the information given in the table to determine the standard free energy of formation vales, Gf° (kJ/mol) for the substance D. 1 A(s) + 1 B(g) → 1 C(s) + 1 D(g) Substance Gf°(kJ/mol) A(s) -684.3 B(g) -223.7 C(s) 187.7

A student determines the value of the equilibrium constant to be 3.88×1013 for the following reaction.4HCl(g) + O2(g)2H2O(g) + 2Cl2(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less)  than zero.Calculate the free energy change for the reaction of 1.80 moles of HCl(g) at standard conditions at 298K.    G°rxn =  kJ

For the reaction CO(g) + 3H2(g) → CH4(g) + H2O(g) AH = -206.1 kJ and AS° = -214.7 J/K The standard free energy change for the reaction of 1.52 moles of CO(g) at 253 K, 1 atm would be This reaction is reactant favored under standard conditions at 253 K. Assume that AH° and AS are independent of temperature. kJ.

Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation of NH3 (g) is -104 kJ/mol at 298 K, calculate the equilibrium constant, K, at this temperature. To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.

A student determines the value of the equilibrium constant to be 6.04x10-37 for the following reaction. 2N2(g) + O2(g) 2N20(g) ht Based on this value of Keg: than zero. AG° for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 2.09 moles of N2(g) at standard conditions at 298K. AG°rxn kJ

The equilibrium constant for the equation       HNO2 (aq)  +  H2O (l)    ⇌    H3O+ (aq)  +  NO2− (aq) is Ka = 5.6 × 10−4 M at 25.0 °C. a) Calculate the value of ΔG°rxn, in kJ/mol, at 25.0 °C. b) Calculate the value of ΔGrxn, in kJ/mol, at 25.0 °C when [NO2−] = [H3O+] = 1.0 ×10−5 M and [HNO2] = 1.00 M.

The equilibrium constant (Kp) for the balanced reaction A(g) + B(g) C(g) + D(g) is Kp = 4.61 at 2000.0 K and the value for the standard free energy of this reaction is -31.5 kJ/mol also at 2000.0 K. What is the value of the non-standard free energy (in units of kJ/mol) for the reaction at the same temperature if the partial pressures of the mixture are: PA = 0.260 atm; Pg = 0.790 atm; Pc= 0.660 atm; and Pp = 1.20 atm Recall: AG= AG° + RT In Q R=8.3144 J/(K mol) Type your answer in the space below without the units.

​ Determine ΔG°rxn for the following reaction:   N2O (g)  +  NO2 (g)  à  3 NO (g)​​ΔG° = ? Use the following reaction with known ΔG° values. ​Rxn 1:​​2 NO (g)  +  O2 (g)  à   2 NO2 (g)​​ΔG1° =  - 71.2 kJ​ ​Rxn 2:​​N2 (g)  +   O2 (g)  à   2 NO (g)​​ΔG2° =  + 175.2kJ Rxn 3:​​2 N2O (g)   à   2 N2 (g)  +   O2 (g)  ​​ΔG3° =  - 207.4kJ