Which of the following represents a balanced half-reaction for the following whenbalanced in acidic conditions?MnO2(aq) → Mn²(aq)SH+MnO,(aq)→→ Mn2+ (aq) + 4H₂O(el) + Se-SH*+MnO2(aq) + 7e → Mn²+ (aq) + 4H₂O(el)SH*+MnO2(aq) + Se →Mn²+ (aq) + 4H₂O(el)4H* + MnO2(aq) + 3e → Mn2+ (aq) + 2H₂O(el)SH*+MnO(aq) → Mn(aq) + 4H₂O(el) + 7e-Identify the reducing agent in the reaction:Ag(s) + NO3(aq) → Ag* (aq) + NO(g)NO₂(aq)there is no reducing agentAg+ (aq)Ag (s)ONO(g)Identify the reducing agent in the reaction:2Fe(s) + O₂(g) + 2 H₂O(el) →2Fe(OH), (s)H₂O(el)0₂ (8)Fe(OH), (s)Fe(s) and O₂(g)Fe(s)O O O O O

According to Bartlby guidlines I solve only first question. You post other two questions separately.

Which of the following represents a balanced half-reaction for the following when balanced in acidic conditions? MnO(aq) → Mn* (aq) SH+MnO(aq) → Mn2+ (aq) + 4H₂O(el) + Se SH+MnO(aq) + 7e → Mn³ (aq) + 4H₂O(el) SH+MnO(aq) + Se → Mn2(aq) + 4H₂O(el) 4H*+MnO(aq) + 3e → Mn²(aq) + 2H₂O(el) SH*+MnO(aq) →→ Mn2+ (aq) + 4H₂O(el) + 7e-

Which of the following represents a balanced half-reaction for the following when balanced in acidic conditions? MnO(aq) → Mn* (aq) SH+MnO(aq) → Mn2+ (aq) + 4H₂O(el) + Se SH+MnO(aq) + 7e → Mn³ (aq) + 4H₂O(el) SH+MnO(aq) + Se → Mn2(aq) + 4H₂O(el) 4H+MnO(aq) + 3e → Mn²(aq) + 2H₂O(el) SH+MnO(aq) →→ Mn2+ (aq) + 4H₂O(el) + 7e-

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Balance the following redox reaction in acidic solution. 2+ Fe²+ (aq) + MnO₂(s) ->> 3+ 2+ Fe (aq) +Mn (aq)
[3] Balance the following redox reaction in basic solution. Sb;O;(s) + NO; (aq) → H;SbO4(aq) + NO(g)
Balance the following skeleton reaction and identify the oxidizing and reducing agents: MnO4−(aq) + HCOOH(aq) → Mn2+(aq) + CO2(g) [acidic]
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: (aq) + 2Cu+ (aq) → Pb(s) + 2Cu²+ (aq) AG° Pb²+ = Pb²+ (aq) + 2e¯ → Pb(s) Ee = -0.126 V red 2+ Cu²+ (aq) + e → Cu+ (aq) Fº red kJ K for this reaction would be = = 0.153 V + than one.
Write oxidation and reduction half reactions for the following: Fe2+(aq) + MnO4-(aq) → Fe3+(aq) + Mn2+(aq)
Balance the following redox equation to its lowest integer ratio. (Under Acidic Conditions) Te(s) + Ru(NO3)3(aq) + NO2(g) ↔ Ru2Te3(s) + HNO3(aq) Note that H2O and H+ are not shown in the equation above. If it is required to balance the equation, then add these.Fill in the coefficient for each chemical after you finish balancing the equation. If the chemical is not needed in the equation then mark a zero next to it Te(s) HNO3(aq) H2O(l) Ru2Te3(s) NO2(g) Ru(NO3)3(aq) H+ (aq)
Complete and balance the following half-reaction in basic solution 5 X Cr(OH)3(s) → CrO42-(aq)
Using data in the Table, what is the equilibrium constant for the reaction: 2Fe 3+(aq)+H 2(g) 2Fe 2+(aq) + 2H +(aq)?
For the following redox reaction, write a balanced equation for the whole reaction and include the states of matter: MnO4 (aq) + Cl (aq) → Mn²+ (aq) + Cl₂(g) (in acidic solution) Balanced equation: ->>>
Balance the redox reaction in acidic solution. Y(s) + XO, (aq)→ YO(s) + XH3(aq)
Complete and balance the following half-reaction in basic solution Cr(OH)₃(s)→CrO₄²⁻(aq)