the balanced reaction in acidic medium is I2 + H2S ---> 2I-+S+2H+. Should I place (s) in S? For instance, I2 + H2S ---> 2I-+S (s) +2H+. Which is the correct answer?
the balanced reaction in acidic medium is I2 + H2S ---> 2I-+S+2H+. Should I place (s) in S? For instance, I2 + H2S ---> 2I-+S (s) +2H+. Which is the correct answer?
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...
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Good day! I have a question regarding
In letter b, the balanced reaction in acidic medium is I2 + H2S ---> 2I-+S+2H+.
Should I place (s) in S?
For instance, I2 + H2S ---> 2I-+S (s) +2H+.
Which is the correct answer?
![个
Step 3
(b).
Balanced oxidation-half is:
H₂S-
----> S + 2H+ + 2e¯
Balanced reduction-half is:
1₂ +2e
--> 21¯
Add both the equations.
So,
Balanced reaction in acidic medium is :
12 + H₂S
--> 21¯ + S + 2H+
Oxidizing agent is the agent which undergoes
reduction. Therefore, oxidizing agent = 1₂
Reducing agent is the agent which undergoes
oxidation. Therefore, reducing agent = H₂S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9289afb0-bf87-42c4-b10b-16e3ec0f403c%2Fd47907e7-8bc9-49d6-a58e-8a384df90999%2F20ps6cl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:个
Step 3
(b).
Balanced oxidation-half is:
H₂S-
----> S + 2H+ + 2e¯
Balanced reduction-half is:
1₂ +2e
--> 21¯
Add both the equations.
So,
Balanced reaction in acidic medium is :
12 + H₂S
--> 21¯ + S + 2H+
Oxidizing agent is the agent which undergoes
reduction. Therefore, oxidizing agent = 1₂
Reducing agent is the agent which undergoes
oxidation. Therefore, reducing agent = H₂S
![2+
(a) MnO4 + VO²+ → Mn²+ + V(OH)4
(b) I₂ + H₂S(g) → I¯¯ +S(s)
2+
(c) Cr₂O7²- + U4+ → Cr³+ + UO₂²+
(d) Cl + MnO₂ (s) → Cl₂(g) + Mn²
(e) IO3 + I→→ 1₂(aq)
(f) IO3 + I + Cl¯ → IC¹₂
(g) HPO3²- + MnO4 + OH → PO³+ MnO2-
Write balanced redox equations for the following
reactions. Show the full balancing process and supply H+
and/or H2O as needed to obtain balance. Item g is
balanced in basic medium while the rest are in acidic
medium. Identify the oxidizing agent and the reducing
agent on the left side of each equation in the previous
problem.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9289afb0-bf87-42c4-b10b-16e3ec0f403c%2Fd47907e7-8bc9-49d6-a58e-8a384df90999%2Fe914wmp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:2+
(a) MnO4 + VO²+ → Mn²+ + V(OH)4
(b) I₂ + H₂S(g) → I¯¯ +S(s)
2+
(c) Cr₂O7²- + U4+ → Cr³+ + UO₂²+
(d) Cl + MnO₂ (s) → Cl₂(g) + Mn²
(e) IO3 + I→→ 1₂(aq)
(f) IO3 + I + Cl¯ → IC¹₂
(g) HPO3²- + MnO4 + OH → PO³+ MnO2-
Write balanced redox equations for the following
reactions. Show the full balancing process and supply H+
and/or H2O as needed to obtain balance. Item g is
balanced in basic medium while the rest are in acidic
medium. Identify the oxidizing agent and the reducing
agent on the left side of each equation in the previous
problem.
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