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Chapter 17: Problem 48

Write the balanced half-reaction for the conversion of \(\mathrm{Cl}_{2}(g)\) to \(\mathrm{Cl}^{-}(a q) .\)

Short Answer

Expert verified
The balanced half-reaction for the conversion of \(\mathrm{Cl}_{2}(g)\) to \(\mathrm{Cl}^{-}(a q)\) is \(\mathrm{Cl}_{2}(g) + 2e^{-} \rightarrow 2 \mathrm{Cl}^{-}(a q)\)

Step by step solution

01

- Write the Unbalanced Equation

The unbalanced equation describes what happens in the reaction. Write down the reaction of changing \(\mathrm{Cl}_{2}(g)\) into \(\mathrm{Cl}^{-}(a q)\): \[ \mathrm{Cl}_{2}(g) \rightarrow \mathrm{Cl}^{-}(a q) \]
02

- Balance Atoms

In the unbalanced equation, there are two Cl atoms on the reactant-side, but only one Cl atoms on the product-side. To balance the chlorine atoms in our reaction, the Cl- side needs two atoms: \[ \mathrm{Cl}_{2}(g) \rightarrow 2 \mathrm{Cl}^{-}(a q) \]
03

- Balance Charges

Now, it's time to balance the charges. You have a neutral molecule on the reactant-side and on the product-side you have two negatively charged ions. To make both sides have equal charges, we need to add 2 electrons to the reactant-side to balance the 2 negative charges that appear on the product-side: \[ \mathrm{Cl}_{2}(g) + 2e^{-} \rightarrow 2 \mathrm{Cl}^{-}(a q) \] This is the balanced half-reaction.

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