Ni(s) | Ni2+(aq) Ag+(aq) | Ag(s)
If you mean a reaction of AgNO3 + Na(s) ==> NaNO3 + Ag(s), there would be ONE electron transferred.Ag^+ + 1e- ==> Ag(s) Reduction reaction Na(s) ==> Na^+ + 1e- Oxidation reaction
The reaction is:Ag+ + Cl- = AgCl(s)Silver chloride is an insoluble, white, photosensitive precipitate.
Ag(s)
The mass of 2,65 Ag moles is 285,85 g.
2hno3+3h2s --> 3s+2no+4h2o
ag is + s is -2
Ag+(aq) + e- → Ag(s) and Cu(aq) → Cu2+(aq) + 2e-
Fe(s) + 3AgNO3 ---> Fe(NO3)3 + Ag(s) The oxidation # of Ag on the left is 1+ and on the right it is zero. It has gained electrons and has been reduced.
Net Ionic: Cd^+2+(aq) + S^2-(aq) ==> CdS(s)The Na^+ and Cl^- are spectator ions.
Cd^2+(aq) + 2Cl^-(aq) +2Na^+(aq) + S^2-(sq) ==> CdS(s) + 2Na^+(aq) + 2Cl^-(aq)The 2Na^+(aq) and the 2 Cl^-(aq) are spectator ions as they appear on both sides of the equation. Thus, the NET reaction is ...Cd^2+(aq) + S^2-(aq) ==> CdS(s)What else was your question. This is classed as a double replacement reaction.
Carbon dioxide and water. 2HNO3(aq) + CaCO3(s) => Ca(NO3)2 (aq) + H2O + CO2
The above reaction is a combination type reaction between silver (Ag) and sulfur (S)
Na+ and C2H3O2- (acetate) don't react. Only Ag+ and Cl- do so by precipitation: Ag+ + Cl- --> (AgCl)s
Ni(s) | Ni2+(aq) Ag+(aq) | Ag(s)
1 mol Ag/ 107.87g Ag ---/---------------------------------------- x2=215.74g Ag / 1mol Ag 1 mol S/32.07g S --------/------------------------------------32.07g S /1 mol S total=247.81g Ag2S 215.47g Ag/247.81=.8706 87.06% Ag .8706 or 87.06% Ag x 125g Ag2S = 108.83g Ag can be produced from Ag2S
If you mean a reaction of AgNO3 + Na(s) ==> NaNO3 + Ag(s), there would be ONE electron transferred.Ag^+ + 1e- ==> Ag(s) Reduction reaction Na(s) ==> Na^+ + 1e- Oxidation reaction