Question
Asked Dec 3, 2019
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The following change occurs in acidic solution:

____ S2–(aq) + ____ Cr2O72–(aq) → ____ S(s) + ____ Cr3+(aq)

In the balanced equation, for every mole of Cr2O72– that reacts, _____ mol of H+ are consumed.

a. 7

b. 14

c. 5

d. 10

e. 8

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Expert Answer

Step 1

The given reaction is,

s* (aq) + C;O; (aq) स्टे S( s ) + Cr " (aq)
C;O; (aq) स्टे s(s )
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Image Transcriptionclose

s* (aq) + C;O; (aq) स्टे S( s ) + Cr " (aq) C;O; (aq) स्टे s(s )

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Step 2

Step (1): separate the above reaction into two half reactions and balance all other atoms except hydrogen and Oxygen.

Oxidation half-reaction: S (aq)
S(s)
+2e
Reduction half-reaction: Cr2 O (aq) +6e -2 Cr3* (aq)
help_outline

Image Transcriptionclose

Oxidation half-reaction: S (aq) S(s) +2e Reduction half-reaction: Cr2 O (aq) +6e -2 Cr3* (aq)

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Step 3

Step (2): Balance the charge by adding H+ ion and balance the Oxygen by add...

Oxidation half-reaction: 3S2 (aq) -» 3S(s) +6e
Reduction half-reaction: Cr2 O (aq) +6e 14H ->2Cr (aq) 7H,O
help_outline

Image Transcriptionclose

Oxidation half-reaction: 3S2 (aq) -» 3S(s) +6e Reduction half-reaction: Cr2 O (aq) +6e 14H ->2Cr (aq) 7H,O

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