\( \text{K}_2\text{Cr}_2\text{O}_7 \) is heated with KCl in pressure of \( \text{H}_2\text{SO}_4 \). Find the correct match of product with their oxidation state.
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When reacting \( \text{K}_2\text{Cr}_2\text{O}_7 \) with \( \text{KCl} \) in \( \text{H}_2\text{SO}_4 \), chromium undergoes reduction and chloride acts as a ligand, forming \( \text{CrO}_2\text{Cl}_2 \) with chromium in the +6 oxidation state.
Step 1: Understand the reaction.
When potassium dichromate (\( \text{K}_2\text{Cr}_2\text{O}_7 \)) is heated with potassium chloride (KCl) in the presence of sulfuric acid (\( \text{H}_2\text{SO}_4 \)), the reaction forms \( \text{CrO}_2\text{Cl}_2 \) (chromyl chloride). The chromium in \( \text{CrO}_2\text{Cl}_2 \) is in the +6 oxidation state.
The reaction can be summarized as:
\[
\text{K}_2\text{Cr}_2\text{O}_7 + 6 \, \text{KCl} + 3 \, \text{H}_2\text{SO}_4 \rightarrow 2 \, \text{CrO}_2\text{Cl}_2 + 3 \, \text{K}_2\text{SO}_4 + 3 \, \text{H}_2\text{O}
\]
Step 2: Identify the oxidation states.
In the product \( \text{CrO}_2\text{Cl}_2 \), the oxidation state of chromium is +6, which matches the given option.
Thus, the correct answer is \( \text{CrO}_2\text{Cl}_2 \), with chromium in the +6 oxidation state.
