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Question 55 (1 point) Calculate AGrxn at 398 K under the nonstandard conditions shown below for...
Question 56 (1 point) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 3 Cl2(g) + 2 Fe(s) → 6 (aq) + 2 Fe3+(aq) E° = +1.36 V Cl2(g) + 2 e 2 Cl(aq) Fe3+(aq) + 3 e → Fe(s) E° = -0.04 V O-1.32 V +4.16 V +1.40 V -1.40 V +1.32 V Question 55 (1 point) Calculate AGrxn at...
Calculate ΔGron (kl) at 298 K under the conditions shown below for the following reaction. SO3lg)+ H20(e) -H2SO4() AG--90.5kJ P(SO3)-0.20 atm, P(H20)-0.88 atm Input your answer with one decimal place. No unit
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.20 atm, P(O3) = 0.038 atm kj = ?
Calculate Grxn at 298 K under the conditions shown below for the following reaction. 2 H2S(g) + 3 O2(g) 2 SO2(g) + 2 H2O(g) G°rxn = ? G°f (kJ/mol) -33.4 -300.1 -228.6 P(H2S) = 1.4 atm, P(O2) = 0.5atm P(SO2) = 2.2atm and P(H2O) = 0.8 atm
Calculate the free energy AG at 25°C for the nonstandard conditions at point where the reaction quotient Q is 2.75 x 10 Express your answer numerically in kilojoules. View Available Hint(s) % ALC O ? AG - CO Nitrosyl chloride formation Chlorine gas. Cl(s), reacts with nitric oxide, NO(), to form nitrosyl chloride, NOCI(g), via the reaction Cl(s) + 2NO(g) + 2NOCI() The thermodynamic data for the reactants and products in the reaction are given in the following table: Substance...
Under certain nonstandard conditions, oxidation byO2(g) of 1 mol of SO2(g) to SO3(g) absorbs 89.3 kJ . The heat of formation of SO3(g) is -204.1 kJ/mol under these conditions. Find the heat of formation of SO2(g). [in kJ/mol]
4. Calculate ΔGrn at 298 K under the conditions shown below for the following reaction. 3 02g) 2 Os(g) P(O2) 0.41 atm, P(O) 5.2 atm AGo +326 kJ a. +341 kJ b. +17.8 kJ c. +332 kJ d. -47.4 kJ e. -109 kJ
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.41 atm, P(O3) = 5.2 atm
Calculate AG° (kJ/mole) at 298 K for the reaction below: H2SO4(1) <H2O(1)+ SO3(g) K=2.07 x 10-12 Enter a number to 2 decimal places.
Since the computed value for AG is positive, the reaction is nonspontaneous under these conditions. Check Your Learning Calculate the free energy change for this same reaction at 875 °C in a 5.00 L mixture containing 0.100 mol of each gas. Is the reaction spontaneous under these conditions? ANSWER: AG = +45.1 kJ/mol; no EXAMPLE 16.12 Calculating AG under Nonstandard Conditions What is the free energy change for the process shown here under the specified conditions? T = 25 °C,...