EZ GchemQ

[utdent20]

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Which of the following is the oxidizing agent and the element reduced. in the following: and why?
Sn(s) +HNO3(aq)--->Sn(NO3)2(aq) + H20

 

[JBarr29]

well Sn(s) is going from a 0 charge to a +2 which means its losing e-'s. Loss of electrons is Oxidation. However, nothing is being reduced really because nothing else is gaining electrons. where did you get that problem from?

 

[utdent20]

Its from Top score, the answer is NO3 and N is the element reduced according to the answers.. so i am lost myself.

 

[Danny289]

Which of the following is the oxidizing agent and the element reduced. in the following: and why?
Sn(s) +HNO3(aq)--->Sn(NO3)2(aq) + H20

the correct equation is:
Sn + 4 HNO3 = SnO2 + 4 NO2 + 2 H2O
Now the answer make sense. isn't it?
reduxtion and oxidation must happen together. because we have lost and gain electrons together.

 

[joonkimdds]

Which of the following is the oxidizing agent and the element reduced. in the following: and why?
Sn(s) +HNO3(aq)--->Sn(NO3)2(aq) + H20

Sn = 0
HNO3 ==> O = -6, H = 1, thus N = 5
Sn(NO3)2 ==> O = -6, N = 5, combined = -1 then x2 = -2 thus Sn=2
H2O = O = -2, H = 1 each

Sn = 0 to 2 thus oxidized and reducing agent

but....I don't understand which one should be oxidizing agent.

and I don't know what Danny did.

 

[rdhdds1]

Sn = 0
HNO3 ==> O = -6, H = 1, thus N = 5
Sn(NO3)2 ==> O = -6, N = 5, combined = -1 then x2 = -2 thus Sn=2
H2O = O = -2, H = 1 each

Sn = 0 to 2 thus oxidized and reducing agent

but....I don't understand which one should be oxidizing agent.

and I don't know what Danny did.

I am lost as well

 

[Maygyver]

Sn = 0
HNO3 ==> O = -6, H = 1, thus N = 5
Sn(NO3)2 ==> O = -6, N = 5, combined = -1 then x2 = -2 thus Sn=2
H2O = O = -2, H = 1 each

Sn = 0 to 2 thus oxidized and reducing agent

but....I don't understand which one should be oxidizing agent.

and I don't know what Danny did.

I think the OP just posted the wrong question.

 

[Danny289]

Sn = 0
HNO3 ==> O = -6, H = 1, thus N = 5
Sn(NO3)2 ==> O = -6, N = 5, combined = -1 then x2 = -2 thus Sn=2
H2O = O = -2, H = 1 each

Sn = 0 to 2 thus oxidized and reducing agent

but....I don't understand which one should be oxidizing agent.

and I don't know what Danny did.

I am lost as well

the equation in original question doesn't make sense.

Sn=======> Sn+2 + 2e
that means Sn oxidized you right about that.
also H=1 O=-2 and N= +5 in both sides of equation. nothing is (are)reduced! and it is not possible, you must have both reduction and oxidizing. Thus the equation is wrong. i wrote correct one in my post.
good luck guys. 👍

 

[utdent20]

its the right equation..from the topscore version.

 

[Electrons]

Which of the following is the oxidizing agent and the element reduced. in the following: and why?
Sn(s) +HNO3(aq)--->Sn(NO3)2(aq) + H20

Sn is oxidizing agent since it is going from 0 to +2
Since Sn is oxidized, somebody has to reduce, it has to be (NO3)2 in the product side since it is attached to Sn? That would be my logic.

 

[Danny289]

Sn is oxidizing agent since it is going from 0 to +2
Since Sn is oxidized, somebody has to reduce, it has to be (NO3)2 in the product side since it is attached to Sn? That would be my logic.

your logic is right but NO3 reduced in this equation?

 

[Electrons]

your logic is right but NO3 reduced in this equation?

I know what you are saying, it's usually the complement specie, but O & H in H2O is still same ox state. In NO3, it's also same state for N & O as before and after.

Only S changes and so I figure no better answer but the other combining anion to the S must be the recieving of extra losing e- ox state from S?

 

[joonkimdds]

wait...so does this question have an error or no?