How do you write the balanced molecular and net ionic equations for the reaction between aluminum metal and silver nitrate? What are the oxidation and reduction half-reactions?

Answer 1

Well, #"silver nitrate"# is reduced..........

#Ag^(+) + e^(-) rarr Ag(s)darr#

Additionally, aluminum oxidizes.

#Al(s) rarr Al^(3+) + 3e^(-)#

Additionally, we add the half equations to get rid of the electrons.

#Al(s) +3Ag^(+) rarrAl^(3+) + 3Ag(s)#

Similarly.

#Al(s) +3AgNO_3(aq) rarrAl(NO_3)_3(aq) + 3Ag(s)#
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Answer 2

The balanced molecular equation for the reaction between aluminum metal and silver nitrate is:

[2Al_{(s)} + 3AgNO_{3(aq)} \rightarrow 2Al(NO_3)3(aq) + 3Ag{(s)}]

The net ionic equation for the reaction is:

[2Al_{(s)} + 6Ag^+{(aq)} + 6NO{3(aq)}^- \rightarrow 2Al^{3+}{(aq)} + 6NO{3(aq)}^- + 3Ag_{(s)}]

The oxidation half-reaction is:

[2Al_{(s)} \rightarrow 2Al^{3+}_{(aq)} + 6e^-]

The reduction half-reaction is:

[6Ag^+{(aq)} + 6e^- \rightarrow 3Ag{(s)}]

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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 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 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 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.

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