The correct answer is (3)\(A: CrO_2Cl_2\) and \(B: Na_2CrO_4\). The reaction involves the mixture of \(K_2Cr_2O_7\) (potassium dichromate) and \(NaCl\) (sodium chloride) being warmed with concentrated \(H_2SO_4\) (sulfuric acid). The chemical equation is as follows: \[ 2K_2Cr_2O_7 + 8NaCl + 6H_2SO_4 \rightarrow 2CrO_2Cl_2 + 2K_2SO_4 + 8NaHSO_4 + 3H_2O \] Here's a step-by-step explanation: 1. Formation of Chromyl Chloride (\(CrO_2Cl_2\)): \(K_2Cr_2O_7\) is a powerful oxidizing agent. When it reacts with \(H_2SO_4\), it gets reduced. The chromium in the \(K_2Cr_2O_7\) changes its oxidation state from +6 to +4, forming \(CrO_2Cl_2\), which is a red-orange volatile compound known as chromyl chloride.
2. Reaction Overview: \(2K_2Cr_2O_7 + 8NaCl + 6H_2SO_4 \rightarrow 2CrO_2Cl_2 + 2K_2SO_4 + 8NaHSO_4 + 3H_2O\)
3. Chromyl Chloride (\(CrO_2Cl_2\)) in the Presence of Moist \(NaOH\): Chromyl chloride reacts with moist \(NaOH\) to form yellow sodium chromate (\(Na_2CrO_4\)): \[ CrO_2Cl_2 + 2NaOH \rightarrow Na_2CrO_4 + 2HCl \] The yellow color of sodium chromate imparts a yellowish tint to the solution.
In summary, the red vapors of \(CrO_2Cl_2\) are evolved during the reaction with \(K_2Cr_2O_7\) and \(NaCl\) in the presence of concentrated \(H_2SO_4\). When these vapors react with moist \(NaOH\), they form yellowish sodium chromate (\(Na_2CrO_4\)). Therefore, \(A\) is \(CrO_2Cl_2\) (chromyl chloride), and \(B\) is \(Na_2CrO_4\) (sodium chromate).
So, the correct answer is: 3. \(A: CrO_2Cl_2\) and \(B: Na_2CrO_4\) |