I would love some input on a few problems, listed below. My answers follow the questions
1. Would it be feasable to store a solution of lead nitrate in a container of metallic zinc? Why or why not?
No, it would not. A chemical reaction takes place, as the lead oxidizes the zinc.
2. Would it be feasable to store a solution of lead sulfate in a container of metallic silver? Why or why not?
no idea.
3. Would you expect jewelry made of an alloy of silver or copper to tarnish (react) in an environment where chlorine fumes were present?
Yes, because it is a strong oxidizing agent.
You need to look up the activity series in your text. Here is a web site for it.
http://en.wikipedia.org/wiki/Reactivity_series
1. Correct. Zn will go into solution and lead (II) ion will come out; basically, the container will dissolve.
2. Look at the activity series. A metal will displace an ion below it. Notice in problem 1 that Zn is above Pb. In this one, Ag is below Pb.
3. Your answer is correct BUT you didn't expand on your answer; some profs might think you were trying to guess your way through the question. You might want to write the equation for the reaction between Ag and Cl2 and Cu and Cl2.
1. Since Zn is higher on the activity series than lead, the reaction would be:
Zn(s) + Pb(NO3)2(aq) ---> ZnCl2(aq) + Pb(s)
The zinc container would dissolve displacing Pb from the solution. Not a good choice of container.
2. Ag(s) + PbSO4(aq) ---> No reaction
(Ag is lower on the activity series than Pb so it will not displace it.)
3. The answer depends on how differently the alloy behaves than the pure metal. Pure copper does react vigorously with Cl2 gas to form CuCl2. A copper alloy might not react as vigorously or may not react at all.
I would not expect silver metal to react with chlorine fumes, especially when alloyed. Some reaction may occur at the surface may occur but I would not expect it to continue rapidly enough for significant tarnishing.
Most tarnishing reactions involve a metal sulfide forming at the surface which is dark and quite visible.
thank you guys so much!!!!!
In order to provide input on the problems you mentioned, let's break down each question and explain how to arrive at the answer:
1. Would it be feasible to store a solution of lead nitrate in a container of metallic zinc?
To determine if it would be feasible to store a solution of lead nitrate in a container of metallic zinc, you need to consider the reactivity of zinc with lead nitrate. Zinc is more reactive than lead, so it can displace or replace the lead in the compound. This means that a chemical reaction could occur between the zinc and lead nitrate, causing the lead to oxidize and the zinc to be displaced. This is not desirable for storing lead nitrate, so the answer would be no, it would not be feasible.
2. Would it be feasible to store a solution of lead sulfate in a container of metallic silver?
To answer this question, you need to consider the reactivity of silver with lead sulfate. Silver is less reactive than lead, so it cannot displace or replace the lead in the compound. Therefore, there should be no significant chemical reaction between silver and lead sulfate. However, it's always beneficial to double-check your answer by referring to reliable chemical references or consulting experts in the field.
3. Would you expect jewelry made of an alloy of silver or copper to tarnish (react) in an environment where chlorine fumes were present?
To determine if jewelry made of silver or copper alloy would tarnish in the presence of chlorine fumes, you need to consider the reactivity of chlorine with these metals. Chlorine is a strong oxidizing agent and can react with both silver and copper. These reactions can lead to the formation of tarnish compounds on the surface of the jewelry. Therefore, you would expect the jewelry to tarnish in an environment where chlorine fumes are present.
It is worth noting that these answers are based on principles of chemical reactivity, and in any practical scenario, it's always important to conduct thorough research or seek professional advice to ensure accuracy and safety.