[Joules23]

can some check my answer for Number 4 (a) and (b)


Also for #3 nitrogen is the reducing agent, because oxygen is the one being reduced, am i correct on that?

[Borek]

dinitrogen pentoxide.

Check out potassium arsenate formula.

[Joules23]

#3
2N + 5O -> N2O5
that was a stupid mistake.. thanks!

Potassium arsenate formula is K3(AsO4)

PB(NO3) + k3(AsO4) -> PB(AsO4) + K3(NO3)

That doesnt equal out, because of the charges.. the only way i could equal them out is how i wrote it.. is both 4 (a) and (b) wrong?

[AWK]

#3
2N + 5O -> N2O5
that was a stupid mistake.. thanks!

Potassium arsenate formula is K3(AsO4)

PB(NO3) + k3(AsO4) -> PB(AsO4) + K3(NO3)

That doesnt equal out, because of the charges.. the only way i could equal them out is how i wrote it.. is both 4 (a) and (b) wrong?

2N₂+5O₂=2N₂O₅
3Pb(NO3)4 + 4K3AsO4=Pb3(AsO4)4+12KNO3
Use brackets for groups only if at least two group exist in formula

[Joules23]

http://en.wikipedia.org/wiki/Dinitrogen_pentoxide
Shows dinitrogen pentoxide as N2O5.. so why wouldnt that be my product instead of 2NO5?
2N2O5 has Nitrogen as +20 and oxygen as -20
N2O5 has Nitrogen as +10 and oxygen as -10

Oh and how does my Net ionic look?

[Borek]

http://en.wikipedia.org/wiki/Dinitrogen_pentoxide
Shows dinitrogen pentoxide as N2O5.. so why wouldnt that be my product instead of 2NO5?

Huh? N₂O₅ IS your product. Two molecules of it per reaction equation.

Oh and how does my Net ionic look?

OK

[Joules23]

this is what im not understanding:
You say this is what i should have:
2N₂+5O₂=2N₂O₅

But why wouldnt it be this:
2N+5O=N₂O₅

is it because Oxygen and Nitrogen are never alone, and always in pairs?

same thing goes for H, F, I, Cl, Br ?

[Borek]

is it because Oxygen and Nitrogen are never alone, and always in pairs?

same thing goes for H, F, I, Cl, Br ?

Exactly.