A redox reaction will occur, producing a metal deposit, when a Sn wire is added to which of the following aqueous solutions? Select one: a. Mg($$NO_3$$)$$_2$$ b. Pb($$NO_3$$)$$_2$$ c. Al($$NO_3$$)$$_3$$ d. Ca($$NO_3$$)$$_2$$
Added by Kimberly C.
Close
Step 1
The question asks which of the given aqueous solutions will react with a tin (Sn) wire to produce a metal deposit. This is a single displacement redox reaction. For a reaction to occur and produce a metal deposit, the tin metal must be more reactive than the metal Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 100 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Predict which of the following metals reacts with aqueous copper(II) nitrate. (a) $\mathrm{Ag}$ (b) Sn (c) $\mathrm{Co}$ (d) $\mathrm{Mn}$
Adi S.
Based on the activity series, which one of the reactions below will occur? A) SnBr2 (aq) + Cu (s) → CuBr2 (aq) + Sn (s) B) Pb (s) + NiI2 (aq) → PbI2 (aq) + Ni (s) C) Mn (s) + NiCl2 (aq) → MnCl2 (aq) + Ni (s) D) Fe (s) + ZnCl2 (aq) → FeCl2 (aq) + Zn (s) E) None of the reactions will occur.
Madhur L.
Use Table $6.3$ to predict whether the following displacement reactions should occur. If no reaction occurs, write N.R. If a reaction does occur, write a balanced chemical equation for it. (a) $\mathrm{Zn}+\mathrm{Sn}^{2+} \longrightarrow$ (d) $\mathrm{Zn}+\mathrm{Co}^{2+} \longrightarrow$ (b) $\mathrm{Cr}+\mathrm{H}^{+} \longrightarrow$ (e) $\mathrm{Mn}+\mathrm{Pb}^{2+} \longrightarrow$ (c) $\mathrm{Pb}+\mathrm{Cd}^{2+} \longrightarrow$
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD