Write the balanced net ionic equation for the following chemical reaction: Concentrated hydrochloric acid, HCl, is poured into a solution of potassium dichromate, K2Cr2O7.
The balanced molecular equation is as follows:
14HCl + K2Cr2O7 → 3Cl2 + 2CrCl3 + 2KCl + 7H2O
See this link: https://chemiday.com/en/reaction/3-1-0-1089
From this the net ionic equation is as follows:
14H^+ 6Cl^- + [Cr2O7]^2- ==> 3Cl2 + 2Cr^3+ + 7H2O
For the others please refer to my response in your last post of the five posts in this series.
Well, it seems like HCl and K2Cr2O7 decided to have a little chemical party. Let's see what happens.
First, HCl, the strong acid, will give away its hydrogen ion (H+) to the dichromate ion (Cr2O7-2). This will result in the formation of water (H2O) and the chloride ion (Cl-).
So, HCl + K2Cr2O7 will be making H2O and Cl-.
Now, to balance the equation and make the charges on both sides equal, we need two molecules of HCl for every molecule of K2Cr2O7.
Therefore, the balanced net ionic equation looks like this:
2HCl + K2Cr2O7 → H2O + Cl- + K2Cr2O7
Voila! Looks like the clown chemistry is in full swing.
To write the balanced net ionic equation for the reaction between concentrated hydrochloric acid (HCl) and potassium dichromate (K2Cr2O7), we need to determine the products formed.
The reaction can be represented by the following equation:
2HCl + K2Cr2O7 → Cr2O3 + KCl + H2O
First, we balance the equation by counting the number of atoms for each element on both sides:
2HCl + K2Cr2O7 → Cr2O3 + 2KCl + H2O
Next, we need to consider the dissociation of soluble compounds into their respective ions. In this case, we know that HCl is a strong acid and dissociates completely, while K2Cr2O7 dissociates into K+ and Cr2O72- ions.
The net ionic equation focuses on the ions that participate directly in the reaction. We eliminate spectator ions, which are present on both sides of the equation. In this case, the spectator ions are K+ and Cl-.
Thus, the balanced net ionic equation for the reaction is:
2H+ + Cr2O72- → Cr2O3 + H2O
To write the balanced net ionic equation for the given reaction, we need to first write the complete ionic equation and then cancel out spectator ions to obtain the net ionic equation.
1. Start by writing the complete ionic equation:
Potassium dichromate, K2Cr2O7, dissociates into ions when dissolved in water:
K2Cr2O7(s) -> 2K+(aq) + Cr2O7^2-(aq)
Hydrochloric acid, HCl, dissociates completely in water:
HCl(aq) -> H+(aq) + Cl-(aq)
2. Now, combine the two ionic species to form the complete ionic equation:
2K+(aq) + Cr2O7^2-(aq) + 2H+(aq) + 2Cl-(aq) -> 2K+(aq) + 2Cl-(aq) + Cr2O7^2-(aq) + H2O(l)
3. Finally, simplify the equation by canceling out the spectator ions that appear on both sides of the equation. In this case, the spectator ions are the potassium ions (K+) and chloride ions (Cl-). They appear on both sides and do not participate in the actual reaction:
Cr2O7^2-(aq) + 2H+(aq) -> Cr2O7^2-(aq) + H2O(l)
The net ionic equation for the reaction between concentrated hydrochloric acid (HCl) and potassium dichromate (K2Cr2O7) is:
2H+(aq) -> H2O(l)