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?
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.
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.
For the first question:
To predict which container would be most suitable for storing the aqueous solution of iron (III) nitrate, we need to consider the reactivity of the metals. Based on the reactivity series of metals, the metal that is higher on the series will be more reactive and therefore capable of replacing the metal in the compound.
The reactivity series from highest to lowest is as follows:
Potassium (K) > Sodium (Na) > Calcium (Ca) > Magnesium (Mg) > Aluminum (Al) > Zinc (Zn) > Iron (Fe) > Lead (Pb) > Hydrogen (H) > Copper (Cu) > Mercury (Hg) > Silver (Ag) > Gold (Au)
In this case, iron is higher on the reactivity series than copper, tin, or silver. Therefore, iron would be the most suitable container for storing the solution of iron (III) nitrate because it is less likely to react with the solution.
For the first question, to determine the most suitable container for storing an aqueous solution of iron (III) nitrate, you need to consider the reactivity of the solution with the container material.
Iron (III) nitrate is an oxidizing agent, which means it has the potential to accept electrons and cause other substances to be oxidized. In this case, it would act as the reducing agent.
To decide which container is most suitable, you need to think about the relative reactivity of the container materials with iron (III) nitrate. The general rule is that a metal higher in the reactivity series will displace a metal lower in the series from its compounds.
The reactivity series is as follows, with the more reactive metals at the top:
Potassium > Sodium > Calcium > Magnesium > Aluminum > Zinc > Iron > Tin > Lead > Copper > Silver > Gold
In this case, iron (III) nitrate contains iron, which is lower in the reactivity series than copper, tin, and silver but higher than iron itself. Therefore, the most suitable container would be silver since it is less reactive than iron.
For the second question, to determine the order of decreasing tendency of the unknown metal, you need to observe its reactions with copper (II) sulfate and zinc nitrate solutions.
If metal X reacts with copper (II) sulfate, plating out copper metal, it means that metal X is more reactive than copper. On the other hand, if metal X does not react with aqueous zinc nitrate, it means that zinc is more reactive than metal X. Therefore, the order of decreasing tendency of the unknown metal can be determined as follows:
Metal X > Copper > Zinc
To further identify the unknown metal, you can consider reactions with other solutions. For example, if metal X reacts with hydrochloric acid, it can indicate the presence of a metal such as magnesium or aluminum. If metal X reacts with nitric acid, it can indicate the presence of a metal such as magnesium, zinc, or iron. By performing additional tests with different solutions, you can narrow down the possibilities and identify the unknown metal more accurately.