1. In the spaces provided, write the correct coefficient for each species when the reaction is properly balanced (acidic solutions). Do not worry about indicating the amount of any H+ or H2O that may be present.
(a) _________Fe2+(aq) + _________Cr2O72–(aq) → ________Fe3+(aq) + _________Cr3+(aq)
(b) __________S8(s) + ______________O2(g) → ___________SO42–(aq)
2. Determine the values of E°cell and ΔG° for the following reactions.
(a) O2(g) + 4 I–(aq) + 4 H+(aq) → 2 H2O(l) + 2 I2(s) E°cell _________ ΔG°__________
(b) 4 IO3–(aq) + 4 H+(aq) → 2 I2(s) + 2 H2O(l) + 5 O2(g) E°cell _________ ΔG°__________
3. Determine the numerical value of Keq at 25 °C for the electrochemical reactions below. I haven’t lectured on this in class, but the “how-to” is clearly illustrated in the textbook in Chapter 19.
(a) PbO2(s) + 4 H+(aq) + 2 Cl–(aq) → ← Pb2+(aq) + 2 H2O(l) + Cl2(g) (acidic solution) Keq____________________________
(b) 3 O2(g) + 2 Br–(aq) → ← 2 BrO3–(aq) (basic solution)
Keq____________________________
Hello, i am sorry to say that as per HOMEWORKLIB RULES experts can answer either only one full question that too first question or first 4 sub-parts like a), b), c) & d) only. I request you to please post remaining question as separate one since my allotted time could not permit me to answer more than one question also. Thank you in advance for your continued support to us.
Really 1a & 1b takes a lot of time, please see below how much work is needed.
Hope this helped you!
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1. In the spaces provided, write the correct coefficient for each species when the reaction is...
Determine the numerical value of Keq at 25 °C for the electrochemical reactions below. I haven’t lectured on this in class, but the “how-to” is clearly illustrated in the textbook in Chapter 19. (a) PbO2(s) + 4 H+(aq) + 2 Cl–(aq) → ← Pb2+(aq) + 2 H2O(l) + Cl2(g) (acidic solution) Keq____________________________ (b) 3 O2(g) + 2 Br–(aq) → ← 2 BrO3–(aq) (basic solution) Keq____________________________
2. Determine the values of E°cell and ΔG° for the following reactions. (a) O2(g) + 4 I–(aq) + 4 H+(aq) → 2 H2O(l) + 2 I2(s) E°cell _________ ΔG°__________ (b) 4 IO3–(aq) + 4 H+(aq) → 2 I2(s) + 2 H2O(l) + 5 O2(g) E°cell _________ ΔG°_________
Balancing Oxidation–Reduction Reactions (Section)Complete and balance the following equations, and identify the oxidizing and reducing agents:(a) Cr2O72-(aq) + I-(aq)→Cr3+(aq) + IO3-(aq) (acidic solution)(b) MnO4-(aq) + CH3OH(aq) →Mn2+(aq) +HCO2H(aq) (acidic solution)(c) I2(s) + OCl-(aq)→IO3-(aq) + Cl-(aq) (acidic solution)(d) As2O3(s) + NO3-(aq)→H3AsO4(aq) + N2O3(aq) (acidic solution)(e) MnO4-(aq) + Br-(aq)→MnO2(s) + BrO3-(aq) (basic solution)(f) Pb(OH)42-(aq) + ClO-(aq)→PbO2(s) + Cl-(aq) (basic solution)
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2 V. Calculate the equilibrium constant (Kc) for the reaction at 298 K. Round your answer to 3 significant figures. H2SO3(aq) + H2O(l) → H2(g) + SO42-(aq) + 2H+(aq) The electrochemical cell described by the cell notation has a standard cell potential of -0.10 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures. Pt(s) l Cr3+(aq),...
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1. Which of the following conditions defines a non-spontaneous oxidation-reduction reaction? E° + ΔG° - Keq <1 E° - ΔG° - Keq <1 E° + ΔG°+ Keq >1 E° + ΔG°- Keq >1 E° - ΔG° + Keq <1 2. What information can be obtained from the Figure below? The equivalence point occurs at pH = 7.0 but the pKa is not known from the graph. Both the pOH and the...
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