Can someone please help me with these? For the net equations, just give a few ex

Question

Can someone please help me with these? For the net equations, just give a few examples using the equations given and explain them, and I can use those examples to learn how to do the rest. Thank you! Can someone please help me with these? For the net equations, just give a few examples using the equations given and explain them, and I can use those examples to learn how to do the rest. Thank you! 3 Write the net ionic equation for al of the reactions observed. If no reaction was observed, then indicate by writing N.R. (for no reaction). Cu+Zn2+ ? Cu +Ap Zn+ Mg Zn + Fe Mg + Fe" ? Mg + AP. ? Al+Fe3+ ? Cu + Mg2 4 Activity Series a eased on your above, list the metals magnesium, iron, copper, zinc, and aluminum, in order of decreasing Which of the metals studied are more active than hydrogen? c Which of the metals studied are less active than hydrogen? d Which of the metals studied would you expect to be most reactive toward oxygen? e Least reactive toward oxygen? f Which metal oxide would you expect to be most easily decomposed by heat, l.e., metai oxide + heat producing the metal + oxygen? 5 If metai X is more active than metal Y (where both elements are in Group D, then indicate which of the following reactions would occur spontaneously Occurs spontaneously? Occurs spontaneously a In the reaction above, what is oxidized? b What is reduced? C What is the oxidizing agent? d What is the reducing agent? 82

Explanation / Answer

Hi do not worry my friend, here you to go

1. Please go through the following standard potential values web page

https://sites.google.com/site/chempendix/potentials

2. Print it and it will be handy whenever required.

Now look at 1st question

Mg + Fe3+ --> ?

look at Standard Reduction Potentials at 298 K of Mg and Fe3+

Fe3+(aq) + 3e– ? Fe(s)     Ered° (V) = -0.04 ---------1

Mg2+(aq) + 2e– ? Mg(s)    Ered° (V) = –2.38 ---------2

look for more negative value Ered° (V) this will become anode and other will be cathode.

Here Mg has more negative Ered° (V) value, hence Mg is anode and Fe3+ is cathode. (Wait look very cleanly whether more negative metal is in neutral state or not, if it is in neutral state then we proceed and write net ionic equation, otherwise no reaction (N.R).

Mg can loose 2 electrons only and becomes Mg2+, but Fe3+ requires 3 electrons, hence we have to balance the reaction interms of electrons, this will be your net ionic equation. Ions are always in (aq) mode and neutral element metal is always in (s) mode ------ aq means aqueous & s means solid.

Net ionic equation: 3 Mg (s) + 2 Fe3+ (aq) --> 3 Mg2+ (aq) + 2 Fe (s)

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Mg + Cu2+ --> ?

Mg2+(aq) + 2e– ? Mg(s)    Ered° (V) = –2.38

Cu2+(aq) + e– ?  Cu+(aq)   Ered° (V) = +0.153

here also Mg is anode and Cu is cathode, no need to balance since both have +2 charges

Net ionic equation: Mg (s) + Cu2+ (aq) --> Mg2+ (aq) + Cu (s)

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Al + Mg2+ --> ?

Mg2+(aq) + 2e– ? Mg(s)    Ered° (V) = –2.38

Al3+(aq) + 3e– ? Al(s)       Ered° (V) = –1.66

here again Mg is anode, but it is in already +2 ionic state, hence it will not lose any more electrons, so NO REACTION between these couples.

Net ionic equation: Al + Mg2+ --> N.R

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Hope this helped you! Still if you have any doubts please use comment section below, but make sure you have tried some equations before asking me for further help, this way you will be self dependent for future problems.

Thank You So Much! Please Rate this answer as you wish.("Thumbs Up")

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