use the activity series to predict if a reaction will occur, complete and and balance your equation.
Zn(s)+ Cu(NO3)2
Well, is Zn more active than Cu? More active means it looses electrons "easier" then Copper? Ans: Yes, Zn looses its electrons to copper. A reaction occurs. Think this out.
To predict whether a reaction will occur using the activity series, we need to compare the reactivity of zinc (Zn) and copper (Cu). The activity series is a list that ranks metals in order of their reactivity, with the most reactive metals at the top and the least reactive metals at the bottom.
Let's consult the activity series to determine the reactivity of zinc and copper. Here is a simplified version of the activity series:
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Cr > Fe > Cd > Ni > Sn > Pb > H2 > Sb > Bi > Cu > Hg > Ag > Pt > Au
We can see that zinc (Zn) is located above copper (Cu) in the activity series. This means that Zn is more reactive than Cu. In other words, Zn will react with Cu(NO3)2.
Now let's complete and balance the equation for the reaction between Zn and Cu(NO3)2:
Zn(s) + Cu(NO3)2(aq) -> Zn(NO3)2(aq) + Cu(s)
In this reaction, zinc (Zn) displaces copper (Cu) from copper nitrate (Cu(NO3)2), leading to the formation of zinc nitrate (Zn(NO3)2) and solid copper (Cu).
Please note that it is important to balance the equation by ensuring that the number of atoms of each element is the same on both sides of the reaction arrow. The balanced equation above satisfies this requirement.