Chemistry: Balancing Redox reactions

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Discussion Overview

The discussion focuses on balancing a redox reaction occurring in acidic solution, specifically involving the reaction between tin (Sn) and permanganate ion (MnO4-). Participants are attempting to verify their balanced chemical equations and are seeking clarification on the correct representation of the species involved.

Discussion Character

  • Homework-related
  • Technical explanation

Main Points Raised

  • One participant presents a balanced equation for the redox reaction and questions its acceptance by their homework system.
  • Another participant agrees that the equation appears correct but suggests ensuring that phases are included in the representation.
  • A third participant reiterates the need for phase notation and provides a similar balanced equation, indicating a potential issue with the formatting of subscripts and superscripts.
  • Another participant proposes that the notation for the permanganate ion may need correction, suggesting it should be represented as MnO4- instead of MnO-4.

Areas of Agreement / Disagreement

Participants generally agree that the balanced equation appears correct, but there are differing views on the proper notation and formatting of the chemical species involved. The discussion remains unresolved regarding the specific formatting issues raised.

Contextual Notes

There are unresolved concerns about the correct placement of subscripts and superscripts in the chemical notation, which may affect the acceptance of the answer in the homework system.

needOfHelpCMath
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What do i have wrong here for my chemical equation? Seems to be right but my homework won't accept it.

Balance the redox reaction occurring in acidic solution.

Sn(s)+MnO−4(aq) → Sn2+(aq)+Mn2+(aq)

Express your answer as a chemical equation including phases.
5Sn+2MnO−4+16H+→5Sn2++2Mn2++8H2O


is this correct?
 
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needOfHelpCMath said:
What do i have wrong here for my chemical equation? Seems to be right but my homework won't accept it.

Balance the redox reaction occurring in acidic solution.

Sn(s)+MnO−4(aq) → Sn2+(aq)+Mn2+(aq)

Express your answer as a chemical equation including phases.
5Sn+2MnO−4+16H+→5Sn2++2Mn2++8H2O


is this correct?

Hi needOfHelpCMath!

It seems correct to me, although the question does ask to include phases.
So should it perhaps be:
$$Sn(s)+MnO^−_4(aq) → Sn^{2+}(aq)+Mn^{2+}(aq)$$
$$5Sn(s)+2MnO^−_4(aq) + 16H^+(aq)→ 5Sn^{2+}(aq)+2Mn^{2+}(aq) + 8H_2O
$$
(Wondering)
 
I like Serena said:
Hi needOfHelpCMath!

It seems correct to me, although the question does ask to include phases.
So should it perhaps be:
$$Sn(s)+MnO^−_4(aq) → Sn^{2+}(aq)+Mn^{2+}(aq)$$
$$5Sn(s)+2MnO^−_4(aq) + 16H^+(aq)→ 5Sn^{2+}(aq)+2Mn^{2+}(aq) + 8H_2O
$$
(Wondering)

So inputed your answer and it said "Check your placement of subscripts and super subscripts"
 
needOfHelpCMath said:
So inputed your answer and it said "Check your placement of subscripts and super subscripts"

Perhaps MnO-4 should be the other way around. That is, it should be MnO4-, since it's really $(MnO_4)^-$. (Thinking)
 

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