A 0.6465 g of bleaching powder Ca(ClO)2 was dissolved in dilute acid and treated with excess potassium iodide the reaction is:
OCl-1 + I-1 + ……. -> Cl-1 + ……. + ……..
1) complete and balance the above reaction .
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OCl-1 + I-1 + ……. -> Cl-1 + ……. + ……..
OCl^- + 2e- + 2H^+ ==> Cl^- + H2O (one half equation)
2I^- ==> I2 + 2e (2nd half equation).
Add the two half equations, cancel the two electrons, and you have the final equation.
To complete and balance the given reaction, we start by identifying the oxidation states of each element involved:
In the compound Ca(ClO)2:
- Calcium (Ca) has a +2 oxidation state.
- Chlorine (Cl) is a halogen, so it has a -1 oxidation state.
- Oxygen (O) normally has a -2 oxidation state, but since there are two chlorine atoms bonded to it, the combined oxidation state of the two chlorine atoms is -1, which means the oxidation state of oxygen is +2.
In the compound potassium iodide (KI):
- Potassium (K) has a +1 oxidation state.
- Iodine (I) is a halogen, so it has a -1 oxidation state.
Now, let's consider the reaction:
OCl-1 + I-1 + .... -> Cl-1 + .... + .....
Based on the oxidation states:
- OCl-1: The chlorine atom has a -1 oxidation state, and the oxygen atom has a +2 oxidation state.
- I-1: The iodine atom has a -1 oxidation state.
- Cl-1: The chlorine atom has a -1 oxidation state.
To balance the reaction, we can set up the following equation:
Ca(ClO)2 + 2KI + H2SO4 -> CaSO4 + 2KCl + I2 + H2O
In this equation, we have balanced the number of atoms on both sides and ensured that the total charges are equal. Additionally, we have included sulfuric acid (H2SO4) as the dilute acid required.
Please note that this balanced equation is a representation of the reaction, but the actual mechanism may involve a series of steps. This balanced equation gives an overall picture of the reaction that occurs.