need help on #5 and #6. Thanks (6 pts) Metals are oxidized into metal cations as
ID: 692668 • Letter: N
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need help on #5 and #6. Thanks
(6 pts) Metals are oxidized into metal cations as they lose electrons and their charge increases. Thus metals are reducing agents. Metal cations are reduced to metal elements (solids except for Hg) as they gain electrons and their charge is reduced to zero. Thus metal cations are oxidizing agents. Answer the following questions about solid 2n, Cu, Pb, Mg, and Ag and their corresponding aqueous ions. Make sure to include (s) or (aq). 5. a) Which is easiest to oxidize? b) Which is hardest to oxidize? c) Which is easiest to reduce? d) Which is hardest to reduce? c) Which is the best reducing agent? f Which is the best oxidizing agent? 6. (4 pts) Assign oxidation numbers for all of the elements in the following redox reaction from a common voltaic cell (batteries). Zeis) , 2Mno,(s1+ 2NH,'(aq) Mn,049 + 2NHfaq) + H:0(l) Element that is oxidized: Oxidizing agent dry cell battery Element that is reduced: Reducing agent: Conclusion: Summarize the electrochemical activity of the metals alone with vour calulated EExplanation / Answer
5) let us arrange the given elements in the order of decreasing reactivity.
Mg > Zn > Pb > Cu > Ag
Among these five Mg, Zn and Pb are above Hydrogen in the reactivity series and Cu and Ag are below hdrogen.
The metals above H in the reactivity series areeasily oxidised into their ions and below H are easily reduced into metals from their ions.
Thus
a) easiest to oxidise is Mg(s) [Mg --> Mg+2 ] is easiest
b) hardest to oxidise is Ag(s) [ Ag to Ag+ is dificult
c) easiest to reduce is Ag+ (aq)
d) hardest to reduce is Mg+2(aq)
e)the best reducing agent is Mg (s) as it readily gives Mg ------> Mg+2 + 2e
f) the best oxidising agent is Ag+(aq)
The reaction Ag+ + e -------> Ag(s) readily takes place
Q6)
The reaction s
Zn + 2 Mn O2 + 2 NH4+ ----------------> Mn2O3 + 2NH3 + Zn+2 + H2O
0 +4 -2 -3 +1 +3 -2 -3 +1 +2 +1 -2 respective oxidation states
Hence the element tat is oxidised is Zn [Zn (0) to Zn(II)]
the element that is reduced is Mn [ +4 to +3]
The oxidising agent is MnO2
the reducing agent is Zn
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