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When the redox equation #Cr^(3+)(aq) + 3Mn(s) -> Mn^(2+)(aq) + Cr(s)# is completely balanced, what will the coefficient of #Cr^(3+)(aq)# be?

Answer 1

Henry Antrim

#2...........#

The oxidation of manganese

#stackrel0Mn(s)rarrMn^(2+) + 2e^(-)# #(i)#

Reduced chromium:

#Cr^(3+) + 3e^(-)rarrstackrel0Cr(s)# #(ii)#

And so we take #3xx(i) + 2xx(ii)# to eliminate the electrons:

#3stackrel0Mn(s)+2Cr^(3+) rarr3Mn^(2+) + 2stackrel(0)Cr#

This is a reasonable representation of reality because charge and mass are balanced. I'm not sure if the reaction works in practice and I'm too lazy to look up redox tables.

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Answer 2

Axel Alvarado

The coefficient of Cr^(3+)(aq) in the balanced redox equation is 1.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When the redox equation #Cr^(3+)(aq) + 3Mn(s) -&gt; Mn^(2+)(aq) + Cr(s)# is completely balanced, what will the coefficient of #Cr^(3+)(aq)# be?

When the redox equation #Cr^(3+)(aq) + 3Mn(s) -> Mn^(2+)(aq) + Cr(s)# is completely balanced, what will the coefficient of #Cr^(3+)(aq)# be?