What I wrote is the balanced ionic equation. The ++ are written as exponents and could be written as we usually do it as
Cu^+2 + Zn ==> Zn^+2 + Cu. For the molecular equation, it is
Cu(NO3)2 + Zn ==> Zn(NO3)2 + Cu
So the ionic equation for adding copper(II)nitrate to pure zinc is:
Cu^2N+Zn---> Zn^2+Cu
then would the balanced equation be:
Cu^2N+Zn---> Zn^2CuN
No. Didn't I write the balanced equation for you yesterday. What is with the ^2N? I know the caret means exponent but what is N?
Cu++ + Zn ==>Zn++ + Cu
I thought I was supposed to add nitrogen to both sides of the equation to balanec it. So is Cu++Zn--->Zn++Cu
the balanced equation for copper(II)nitrate plus pure zinc?
To determine the balanced equation for the reaction between copper(II) nitrate and pure zinc, let's go through the steps for balancing the equation correctly:
1. Start by writing the molecular equation, which represents the overall reaction:
Cu(NO3)2 + Zn -> Zn(NO3)2 + Cu
2. Next, you need to determine the ionic equation by separating the soluble compounds into their respective ions:
Cu^2+ + 2NO3^- + Zn -> Zn^2+ + 2NO3^- + Cu
3. Now, you can cancel out the spectator ions, which appear on both sides of the equation. In this case, the NO3^- ions are spectator ions:
Cu^2+ + Zn -> Zn^2+ + Cu
4. Finally, balance the equation by adjusting the coefficients in front of each compound to ensure that the same number of atoms of each element are present on both sides of the equation:
Cu^2+ + Zn -> Zn^2+ + Cu
The balanced ionic equation for the reaction between copper(II) nitrate and pure zinc is:
Cu^2+ + Zn -> Zn^2+ + Cu