What is the ionic equation for the reaction of chlorine with potassium iodide?
1. Cl2 + 2K → 2KCl
2. 2I⁻ + Cl2 → I2 + 2Cl⁻
3. I⁻ + Cl → I + Cl⁻
4. I⁻ + K+ → KI
2I⁻ + Cl2 → 2Cl⁻ + I2
how?
The reaction between chlorine and potassium iodide can be represented by the following balanced equation:
Cl2 + 2KI → 2KCl + I2
This equation can be split into two half-reactions, one for the oxidation of iodide to iodine and one for the reduction of chlorine to chloride:
I⁻ → I2 + 2e⁻ (oxidation half-reaction)
Cl2 + 2e⁻ → 2Cl⁻ (reduction half-reaction)
By adding these two half-reactions together, the resulting equation is:
2I⁻ + Cl2 → 2Cl⁻ + I2
This is the ionic equation for the reaction between chlorine and potassium iodide.
i dont get it :/
Okay, let me explain it in simpler terms.
When chlorine (Cl2) reacts with potassium iodide (KI), the reaction produces potassium chloride (KCl) and iodine (I2). The balanced equation for the reaction is:
Cl2 + 2Kl → 2KCl + I2
To write the ionic equation, you need to represent the reaction in terms of its ionic species (ions).
The first step is to break apart the ionic compounds KI and KCl into their respective ions:
KI - > K+ + I-
KCl -> K+ + Cl-
Next, you need to identify any ions that don't change during the reaction. In this case, potassium (K+) and chloride (Cl-) ions are spectator ions, which means they don't change during the reaction.
Finally, you need to write the remaining ions as the ionic equation. From the balanced equation, you can see that Iodine (I2) is being formed and Chlorine (Cl2) is being used up. So, the ionic equation is:
2I- + Cl2 → 2Cl- + I2
This equation shows the ionic species that are involved in the reaction.