On heating a mixture of common salt and K_{2} | vedclass

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Question

(B) The reaction between common salt $(NaCl)$, potassium dichromate $(K_{2}Cr_{2}O_{7})$, and concentrated sulfuric acid $(H_{2}SO_{4})$ is as follows

Vedclass · Accepted Answer

$CrO_{2}Cl_{2}$ and $+6$

Vedclass · Answer

(B) The reaction between common salt $(NaCl)$, potassium dichromate $(K_{2}Cr_{2}O_{7})$, and concentrated sulfuric acid $(H_{2}SO_{4})$ is as follows: $4 \ NaCl + K_{2}Cr_{2}O_{7} + 6 \ H_{2}SO_{4}$ $\longrightarrow 2 \ KHSO_{4} + 2 \ CrO_{2}Cl_{2} + 4 \ NaHSO_{4} + 3 \ H_{2}O$ The gas evolved is chromyl chloride $(CrO_{2}Cl_{2})$. In $CrO_{2}Cl_{2}$, let the oxidation state of $Cr$ be $x$. $x + 2(-2) + 2(-1) = 0$ $x - 4 - 2 = 0$ $x = +6$ Thus, the formula is $CrO_{2}Cl_{2}$ and the oxidation state is $+6$.

On heating a mixture of common salt and $K_{2}Cr_{2}O_{7}$ with concentrated $H_{2}SO_{4}$, a gas is evolved. The formula of the gas evolved and the oxidation state of the central metal atom in the gas, respectively, are:

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