In the following situations, a reaction may or may not take place. If it does, write the balanced molecular and total ionic equations illustrating the reaction. Assume all involve aqueous solutions.(a) Some iron nails are placed in a CuCI₂ solution.(b) Silver coins are dropped in a hydrochloric acid solution.(c) A copper wire is placed in a Pb(NO₃)₂ solution.(d) Zinc strips are placed in a Cr(NO₃)₃ solution.
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Metals and reactions
Explanation:
(a) Iron will displace copper from copper sulphate solution. We get iron sulphate and copper.
Fe (Iron) + CuSO4 (Copper Sulphate) → FeSO4 (Iron Sulphate) + Cu (Copper)
(b) Silver does not react with HCl. This is because silver cannot displace hydrogen from HCl. Silver is below hydrogen in the reactivity series and thus cannot displace it.
(c) When copper wire is dipped into solution of lead nitrate, copper being a more reactive metal than lead displaces lead from its compound by forming copper nitrate with a deposit of lead on the copper wire.
(d) Zinc reacts with aqueous chromium as follows:
3Zn(s) + 2Cr3+(aq) → 3Zn2+(aq) + 2Cr(s)"
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