In a lab expirement you add copper(II)nitrate to pure zinc. Write a balanced equation for this expirement and predict if a reaction will occur.
I THINK Bob Pursley answered this question a day or so ago. Zinc is higher in the activity series than copper; therefore, Zn will replace copper ion. Zn goes into solution as Zn(II) and copper(II) comes out of solution to form Cu metal. Repost if there is something about this you don't understand.
I know that a reaction will occur but can you tel me if this balanced equation is correct:
Cu^2N+Zn--->Zn^2+Cu
I'm horrible at chem equations!
Cu^+2 + Zn ==> Cu + Zn^+2 is the ionic equation.
To write the balanced equation for the reaction between copper(II) nitrate and pure zinc, you need to consider the charges and stoichiometry of the elements involved.
The balanced equation is:
Cu(NO3)2 + Zn → Zn(NO3)2 + Cu
Let's break it down to understand the balancing process:
First, identify the formula for copper(II) nitrate, which is Cu(NO3)2. The subscript 2 indicates that there are two nitrate ions present.
Next, write the formula for zinc, which is simply Zn.
Now, balance the equation by ensuring that the number and type of atoms are the same on both sides of the equation. In this case, there is one copper atom and one zinc atom on each side, so no coefficients are needed for these elements.
Moving on, you have two nitrate ions on the left side. To balance the nitrates, you need to place a coefficient of 2 in front of Zn(NO3)2 on the right side to give you a total of four nitrate ions.
The final balanced equation is:
Cu(NO3)2 + Zn → Zn(NO3)2 + Cu
This equation shows that copper(II) nitrate reacts with zinc to form zinc nitrate and copper.
Regarding the prediction of a reaction occurring, as mentioned earlier, zinc is higher in the activity series than copper. This means that zinc is more reactive than copper. In the reaction, zinc will replace the copper ion, resulting in the formation of zinc nitrate and metallic copper. Therefore, a reaction is expected to occur between copper(II) nitrate and pure zinc.