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?
Well,
Additionally, aluminum oxidizes.
Additionally, we add the half equations to get rid of the electrons.
Similarly.
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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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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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