Yes zinc will react to form zinc nitrate and silver.
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∙ 12y agoYes, zinc will react with silver nitrate solution. This reaction occurs because zinc is more reactive than silver, so zinc displaces silver from the silver nitrate solution to form zinc nitrate and silver metal.
When zinc is added to silver nitrate, zinc displaces silver in the reaction, forming zinc nitrate and silver metal. The balanced chemical equation is 2AgNO3 + Zn → Zn(NO3)2 + 2Ag.
Yes, zinc and tin nitrate would react with one another. When zinc is added to tin nitrate solution, a displacement reaction would occur, with the zinc displacing the tin from the nitrate compound to form zinc nitrate and tin metal.
In the reaction between zinc and silver nitrate, zinc displaces silver from the nitrate compound because it is higher in the reactivity series. This displacement reaction results in the formation of zinc nitrate and elemental silver.
When zinc is dipped in silver nitrate, a displacement reaction occurs where zinc atoms replace silver ions in solution. This results in the formation of zinc nitrate and silver metal. The silver metal will coat the surface of the zinc, creating a silver-colored coating.
When acid zinc chloride is added to silver nitrate, a displacement reaction occurs where zinc replaces silver in the compound. This results in the formation of zinc nitrate and silver metal precipitate. The silver metal appears as a solid, while zinc nitrate remains in solution.
When zinc is added to silver nitrate, zinc displaces silver in the reaction, forming zinc nitrate and silver metal. The balanced chemical equation is 2AgNO3 + Zn → Zn(NO3)2 + 2Ag.
Yes, zinc and tin nitrate would react with one another. When zinc is added to tin nitrate solution, a displacement reaction would occur, with the zinc displacing the tin from the nitrate compound to form zinc nitrate and tin metal.
In the reaction between zinc and silver nitrate, zinc displaces silver from the nitrate compound because it is higher in the reactivity series. This displacement reaction results in the formation of zinc nitrate and elemental silver.
Zinc is more reactive than Lead nitrate (See Displacement Series). Therefore, Zinc will displace lead in lead nitrate: Zn + Pb(NO3)2 -> Zn(NO3)2 + Pb
When zinc is dipped in silver nitrate, a displacement reaction occurs where zinc atoms replace silver ions in solution. This results in the formation of zinc nitrate and silver metal. The silver metal will coat the surface of the zinc, creating a silver-colored coating.
When acid zinc chloride is added to silver nitrate, a displacement reaction occurs where zinc replaces silver in the compound. This results in the formation of zinc nitrate and silver metal precipitate. The silver metal appears as a solid, while zinc nitrate remains in solution.
In this reaction, the zinc metal will displace silver ions in the solution because zinc is more reactive than silver. As a result, zinc will oxidize to form zinc ions while silver ions from the silver nitrate will be reduced to form silver metal. This reaction is an example of a single displacement reaction.
Yes, copper would react with zinc nitrate to form copper nitrate and zinc in a single displacement reaction. The zinc would replace the copper in the compound to form zinc nitrate and copper metal.
The product of a single replacement reaction between zinc and silver nitrate is zinc nitrate and silver. The zinc replaces the silver in the compound because it is more reactive, causing a displacement reaction.
Some of the silver ions from the silver nitrate solution are deposited as metallic silver on the contacted parts of the zinc vessel and are replaced by half as many zinc ions in the solution.
Zinc nitrate is formed when nitric acid reacts with zinc. This reaction also produces hydrogen gas.
Yes, zinc can displace nickel from nickel (II) nitrate solution through a single displacement reaction to form zinc nitrate and nickel metal. This reaction occurs because zinc is higher in the reactivity series than nickel, allowing it to replace nickel in the compound.