Write the balanced net ionic equation for the following chemical reaction: A solution of sodium dichromate, Na2Cr2O7, is added to an acidic solution containing Fe2+ ions.
What happened to the Na?
The two balanced half equations are as follows:
Fe^2+ ==> Fe^3+ + e
[Cr2O7]^2- + 6e + 14H^+ ==> 2Cr^3+ + 7H2O
Now you multiply each equation by a number to make the electrons equal; i.e., multiply equation 1 by 6 and multiply equation 2 by 1. Add the two, cancel the electrons and you will have the final net ionic equation.
Na is soluble and disappears because it is a spectator ion
Well, I'm not sure about the "balanced" part, but here's a net ionic equation that's full of chemistry fun:
Fe2+ + Na2Cr2O7 + H+ → Cr3+ + Fe3+ + H2O + Na+ + silly faces
Hope that brings a smile to your face!
To write the balanced net ionic equation for this chemical reaction, we need to follow a few steps:
Step 1: Write the balanced molecular equation.
Na2Cr2O7 + Fe2+ -> Cr3+ + Fe3+ + Na+
In this equation, Na2Cr2O7 reacts with Fe2+ to produce Cr3+, Fe3+, and Na+ ions.
Step 2: Determine the net ionic equation by eliminating the spectator ions.
In this case, the spectator ion is Na+. It does not take part in the reaction and remains unchanged on both sides of the equation.
The net ionic equation is:
Cr2O7^2- + 6Fe2+ -> 2Cr3+ + 6Fe3+
Step 3: Balance the net ionic equation.
To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation.
Cr2O7^2- + 6Fe2+ -> 2Cr3+ + 6Fe3+
This is the balanced net ionic equation for the given chemical reaction.