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5. Consider a reaction starting with reactants and products in nonstandard state conditions, and a negative...
Calculate the free energy AG at 25°C for the nonstandard conditions at point where the reaction...
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...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State wheth...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+...
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+ (aq) → 2H* (aq) + 2 Ag (s) 2H+ + 2e → H2 (g) EⓇ = 0.00V Ag (aq) + le → Ag(s) E = +0.80V a. Write the two half-reactions (oxidation and reduction) occurring in the cell. Clearly indicate which reaction shows oxidation and which shows reduction. Clearly indicate which reaction occurs at the anode and which reaction occurs at the cathode. (4...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) +...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
15. Consider the reaction occurring in a spontaneous electrochemical cell, starting with standard state conditions: Sn(s)...
15. Consider the reaction occurring in a spontaneous electrochemical cell, starting with standard state conditions: Sn(s) + 2H*(aq) → Snº(aq) + H2(g) Which of the following actions would cause the measured cell potential, Ecell, to be greater than Eºcell, (Ecell >Ecell) A. Reducing the mass of the Sn electrode B. Increasing the mass of the Sn electrode C. Increasing the Sn?* ion concentration in the anode compartment. D. Increasing the pressure of hydrogen gas in the hydrogen cell E. Lowering...
1--What is E°cell for the following hypothetical reaction exactly as written (in volts), given the standard...
1--What is E°cell for the following hypothetical reaction exactly as written (in volts), given the standard electrode potential (E°) values below? X(s) + Y2+(aq) → X2+(aq) + Y(s) X2+(aq) + 2 e- → X(s) E° = -0.69 V Y2+(aq) + 2 e- → Y(s) E° = -2.45 V 2--In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as many answers as are correct however points will be deducted for incorrect guesses. Pt(s)|H2(g)|H+(aq)|| Ag(s)|Ag+(aq) Select one...
3. Consider the unbalanced reaction shown below: Au+3 (aq) + Ag (s) Ag+1 (aq) + Au...
3. Consider the unbalanced reaction shown below: Au+3 (aq) + Ag (s) Ag+1 (aq) + Au (s) A. Write out the balanced equation for this reaction. B. What is Eocell for the spontaneous reaction here? C. Give the expression for Q here that would be used in the Nernst equation. D. What is the value of n to be used in Nernst equation here? E. What would be the value of the slope if Ecell were plotted vs log Q...
What is the value of Δ G° (in kJ ) for the following balanced redox reaction at 25.0℃ ?
Half-ReactionE°(V)Fe^(2+)(aq)+2e^(-)rarrFe(s)-0.44Hg^(2+)(aq)+2e^(-)rarrHg(l)0.86Ag^(+)(aq)+e^(-)rarrAg(s)0.80Cu^(2+)(aq)+2e^(-)rarrCu(s)0.34Zn^(2+)(aq)+2e^(-)rarrZn(s)-0.76What is the value of Δ G° (in kJ ) for the following balanced redox reaction at 25.0℃ ?Hg²⁺(a q)+Fe(s) ⟶ Hg(l)+Fe²⁺(a q)a) -40.5 kJb) -81.1 kJc) -125 kJd) -251 kJ
7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for...
7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for this reaction at 1500°C A) 105 kJ/mol B)-105 kJmol C)1.07 kJ/molD) CH,011(g) has the value K, D)255 8) Determine the equilibriurn constant K, at 25°C for the reaction Nag) + 3H2(g) → 2NHO 3 kJ/mol A) 1.52 x 106 B) 6.60 x 10 9) Predict the sign of AS for the reaction 02(g) → 20(g). C) 828 x 10D) 2.60 A) Negative B) zero...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2 pts) a. Use the standard half-cell potentials listed below to calculate the standard cell potential (Eºcell) for 3 Sn(s) + 2 Fe* (aq) - 3 Sn2+ (aq) + 2 Fe(s) Sn 2(aq) + 2 e -Sn (s) E = -0.14 V Fe3+ (aq) + 3 e Fe(s) E° = -0.036 V A) -0.176 V B)-0.104 V C) +0.104 V D) +0.176 V b. Write...
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...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+ (aq) → 2H* (aq) + 2 Ag (s) 2H+ + 2e → H2 (g) EⓇ = 0.00V Ag (aq) + le → Ag(s) E = +0.80V a. Write the two half-reactions (oxidation and reduction) occurring in the cell. Clearly indicate which reaction shows oxidation and which shows reduction. Clearly indicate which reaction occurs at the anode and which reaction occurs at the cathode. (4...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
15. Consider the reaction occurring in a spontaneous electrochemical cell, starting with standard state conditions: Sn(s) + 2H*(aq) → Snº(aq) + H2(g) Which of the following actions would cause the measured cell potential, Ecell, to be greater than Eºcell, (Ecell >Ecell) A. Reducing the mass of the Sn electrode B. Increasing the mass of the Sn electrode C. Increasing the Sn?* ion concentration in the anode compartment. D. Increasing the pressure of hydrogen gas in the hydrogen cell E. Lowering...
7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for this reaction at 1500°C A) 105 kJ/mol B)-105 kJmol C)1.07 kJ/molD) CH,011(g) has the value K, D)255 8) Determine the equilibriurn constant K, at 25°C for the reaction Nag) + 3H2(g) → 2NHO 3 kJ/mol A) 1.52 x 106 B) 6.60 x 10 9) Predict the sign of AS for the reaction 02(g) → 20(g). C) 828 x 10D) 2.60 A) Negative B) zero...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2 pts) a. Use the standard half-cell potentials listed below to calculate the standard cell potential (Eºcell) for 3 Sn(s) + 2 Fe* (aq) - 3 Sn2+ (aq) + 2 Fe(s) Sn 2(aq) + 2 e -Sn (s) E = -0.14 V Fe3+ (aq) + 3 e Fe(s) E° = -0.036 V A) -0.176 V B)-0.104 V C) +0.104 V D) +0.176 V b. Write...
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