3V3+ (aq) + NO3- (aq) + H2O(l) → 3 VO2+ (aq) + NO(g) + 2 H+...
3V3+ (aq) + NO3- (aq) + H2O(l) → 3 VO2+ (aq) + NO(g) + 2 H+ (aq) E° = 0.62 V VO2+ + 2 H+ (aq) + e- → V3+ (aq) + H2O(l) E°= 0.34 V What is E° of nitrate NO3- (aq) + 4 H+ (aq) + 3 e- → NO(g) + 2 H2O(l)
Homework Answers
Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.3...
Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.37 V. Part A Calculate the AGo for the reaction. Express your answer to three significant figures.
Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.37 V. Part A Calculate the AGo for the reaction. Express your answer to three significant figures.
Refer to the following standard reduction half-cell potentials at 25∘C : VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V ...
Refer to the following standard reduction half-cell potentials at 25∘C : VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V Part A Part complete An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.017M)+2H+(aq,1.3M)+e−→→Ni2+(aq,2.5M)+2e−VO2+(aq,2.5M)+H2O(l) Calculate the cell potential under these nonstandard concentrations.
A galvanic cell has the overall reaction: Zn(s) + 2Eu(NO3)3(aq) → Zn(NO3)2(aq) + 2Eu(NO3)2(aq) Which is...
A galvanic cell has the overall reaction: Zn(s) + 2Eu(NO3)3(aq) → Zn(NO3)2(aq) + 2Eu(NO3)2(aq) Which is the half reaction occurring at the anode? (show steps) A) NO3-(aq) + 4H+(aq) + 3e- → NO(g) + 2H2O(l) B) NO2(g) + H2O(l) → NO3-(aq) + 2H+(aq) + e- C) Zn(s) → Zn2+(aq) + 2e- D) Eu3+(aq) + e- → Eu2+ E) Zn(s) + 2e-→ Zn2+(aq)-
Given the following reduction half-reactions: Fe3+(aq)+e−→Fe2+(aq) E∘red=+0.77V S2O2−6(aq)+4H+(aq)+2e−→2H2SO3(aq) E∘red=+0.60V N2O(g)+2H+(aq)+2e−→N2(g)+H2O(l) E∘red=−1.77V VO+2(aq)+2H+(aq)+e−→VO2+(aq)+H2O(l) E∘red=+1.00V Part A Write...
Given the following reduction half-reactions: Fe3+(aq)+e−→Fe2+(aq) E∘red=+0.77V S2O2−6(aq)+4H+(aq)+2e−→2H2SO3(aq) E∘red=+0.60V N2O(g)+2H+(aq)+2e−→N2(g)+H2O(l) E∘red=−1.77V VO+2(aq)+2H+(aq)+e−→VO2+(aq)+H2O(l) E∘red=+1.00V Part A Write balanced chemical equation for the oxidation of Fe2+(aq) by S2O2−6 (aq). Calculate the equilibrium constant K for this reaction at 298 K. Part B Write balanced chemical equation for the oxidation of Fe2+(aq) by N2O(g). Part C Write balanced chemical equation for the oxidation of Fe2+(aq) by VO+2(aq). Calculate the equilibrium constant K for this reaction at 298 K.
Complete and balance the unfinished equations: A) Cu(s) + 4HNO3(aq) ? Cu(NO3)2(aq) + 2NO2(g) +2H20(l) B)...
Complete and balance the unfinished equations: A) Cu(s) + 4HNO3(aq) ? Cu(NO3)2(aq) + 2NO2(g) +2H20(l) B) Cu(NO3)2(aq) +NaOH(aq) ? ? C) Cu(OH)2(s) ? CuO(s) + H2O(l) D) CuO(s) + H2SO4(aq) ? CuSO4(aq) + H2O(l) E) CuSO4(aq) + Zn(s) ? ?
Calculate the E of the cell based on the following half reactions: VO2+ (aq) + 2H+...
Calculate the E of the cell based on the following half reactions: VO2+ (aq) + 2H+ (aq) + e- ----> VO2+ (aq) + H2O (l) Zn (s) --->Zn2+ (aq) + 2e- Under the following condition: T = 25°C [VO2+] = 2.0 M [H+] = 0.5 M [VO2+] = 1.0 x 10-2 M [Zn2+] = 0.10 M
Given the following reduction half-reactions: Fe3+(aq)+e−→Fe2+(aq) E∘red=+0.77V S2O2−6(aq)+4H+(aq)+2e−→2H2SO3(aq) E∘red=+0.60V N2O(g)+2H+(aq)+2e−→N2(g)+H2O(l) E∘red=−1.77V VO+2(aq)+2H+(aq)+e−→VO2+(aq)+H2O(l) E∘red=+1.00V Write balanced chemica
Given the following reduction half-reactions: Fe3+(aq)+e−→Fe2+(aq) E∘red=+0.77V S2O2−6(aq)+4H+(aq)+2e−→2H2SO3(aq) E∘red=+0.60V N2O(g)+2H+(aq)+2e−→N2(g)+H2O(l) E∘red=−1.77V VO+2(aq)+2H+(aq)+e−→VO2+(aq)+H2O(l) E∘red=+1.00V Write balanced chemical equation for the oxidation of Fe2+(aq) by S2O2−6(aq). Calculate ΔG∘ for this reaction at 298 K. Calculate the equilibrium constant Kfor this reaction at 298 K. Write balanced chemical equation for the oxidation of Fe2+(aq) by N2O(g). Calculate ΔG∘ for this reaction at 298 K. Calculate the equilibrium constant Kfor this reaction at 298 K. Write balanced chemical equation for the oxidation of Fe2+(aq)...
Consider the chemical reaction, ClO3−(aq) + 5 Cl−(aq) + 6 H+(aq) ⟶ 3 Cl2(g) + 3 H2O(l)...
Consider the chemical reaction, ClO3−(aq) + 5 Cl−(aq) + 6 H+(aq) ⟶ 3 Cl2(g) + 3 H2O(l) determine if each of the following statements is True or False. 1) Cl2(g) is the reducing agent. [ Select ] ["False", "True"] 2) Cl in ClO3−(aq) gains electrons. [ Select ] ...
You are given the following reduction half reactions in basic solution: 2 NO2-(aq) + 3 H2O(l)...
You are given the following reduction half reactions in basic solution: 2 NO2-(aq) + 3 H2O(l) + 4 e- →N2O(g) + 6 OH-(aq) E° = 0.1500 V HgO(s) + H2O(l) + 2 e- → Hg(s) + 2 OH-(aq) E° = +0.0984 V A. If this redox reaction occurs, how many total electrons will have to be transferred per mole of reaction? N2O(g) + 2 OH-(aq) + 2 HgO(s) → 2 NO2-(aq) + H2O(l) + 2 Hg(s) B. What is the...
(25) What is the phase of Ba(NO3)2 in the following reaction: Ba(OH)2(aq) + HNO3(aq) → Ba(NO3)2...
(25) What is the phase of Ba(NO3)2 in the following reaction: Ba(OH)2(aq) + HNO3(aq) → Ba(NO3)2 + H2O [1] l [2] s [3] aq [4] g [5] ↓
Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.37 V. Part A Calculate the AGo for the reaction. Express your answer to three significant figures.
Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.37 V. Part A Calculate the AGo for the reaction. Express your answer to three significant figures.
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