I don't understand about the "of all the reactants all the ones on the left side......." You may have meant of all the REACTIONS all the METALS on the left side were reducing agents. I think your SRA table is turned around. Shouldn't it be
Mg, Co, Pd? I didn't check the SOA but that should essentially be the reverse of the SRA. Check my thinking. I'll look at the other problems after posting this.
The following equations represent spontaneous reactions. From this evidence, set up a table of relative strengths of oxidizing and reducing agents. Write half-reaction equations and label the strongest oxidizing agent and reducing agent.
Co + Pd2+ ----> Co2+ + Pd
Pd + Pt2+ ----> Pd2+ + Pt
Mg + Co2+ ----> Mg2+ + Co
Of all the reactants all the ones on the left side were reducing agents and I labeled the rest oxidizing agents.
SOA
Pt2+
Pb2+
Co2+
SRA
Pd
Co
Mg
Table
Pe2+ + 2e ---> Pe
Pd2+ + 2e ---> Pd
Co2+ + 2e ---> Co
Mg2+ + 2e ---> Mg
Is that right?
Can someone help me with these questions..
1) A student is required to store an aqueous solution of iron (III) nitrate. She has a choice of a copper, tin, iron, or silver container. Predict wchihc container would be mos suitable for storing the solution.
2) An analytical chemist reacts an unknown metal X with a copper (II) sulfate solution, plating out copper metal. Metal X does not react with aqueous zinc nitrate. What is the order for these metal ions in decreasing tendency of the unknown metal? What other solutions might next be chosen to help identify the unknown metal?
2 answers
1. What is the student guarding against? Does she want to protect the integrity of the iron(III) solution or is she interested only in maintaining the total amount of iron, no matter the species? And I don't know what is meant by suitable, either.
Cu, Sn, and Ag are weaker reducing agents than iron; therefore, the iron(III) solution could be stored in any of them. Ag is the best in my opinion (from a chemical standpoint) BUT Ag is the most expensive AND a silver container might be stolen. I would trade iron for silver any day of the weak. Iron metal would NOT be a good storage for the iron(III) solution because iron metal reacts with iron (III) to produce iron(II). But if the student just wanted to keep the total amount of iron the same then iron would be a good choice because its the cheapest. So you see the answer depends a great deal upon some other knowledge than what has been presented in the problem.
2. X reacts with Cu^+2 to plate out Cu; therefore, X is above Cu. X will not displace Zn+2 so Zn is above X. The series then is
Zn
X
Cu
What metals might we try next. Anything between Zn and Cu; e.g. Cr, Fe, Co, Ni, etc.
Cu, Sn, and Ag are weaker reducing agents than iron; therefore, the iron(III) solution could be stored in any of them. Ag is the best in my opinion (from a chemical standpoint) BUT Ag is the most expensive AND a silver container might be stolen. I would trade iron for silver any day of the weak. Iron metal would NOT be a good storage for the iron(III) solution because iron metal reacts with iron (III) to produce iron(II). But if the student just wanted to keep the total amount of iron the same then iron would be a good choice because its the cheapest. So you see the answer depends a great deal upon some other knowledge than what has been presented in the problem.
2. X reacts with Cu^+2 to plate out Cu; therefore, X is above Cu. X will not displace Zn+2 so Zn is above X. The series then is
Zn
X
Cu
What metals might we try next. Anything between Zn and Cu; e.g. Cr, Fe, Co, Ni, etc.
3 answers