0.004 mol of SO2Cl2(g) is taken in a sealed vessel where it decomposes as SO2Cl2(g)→SO2(g)+Cl2(g) After 0.2303 hours, the gaseous mixture is passed through a 150 ml of acidified, 0.1N I2 (aq) solution where all SO2 is oxidized to SO2−4. The resulting solution of I2 required 90 ml of 0.1 M Na2S2O3(aq) solution.Calculate rate constant (in hr−1) of the reaction. Given : log 2 = 0.3___

0.004 mol of SO2Cl2(g) is taken in a sealed vessel where it decompose

1.	0.004 mol of SO2Cl2(g) is taken in a sealed vessel where it decomposes as SO2Cl2(g)→SO2(g)+Cl2(g) After 0.2303 hours, the gaseous mixture is passed through a 150 ml of acidified, 0.1N I2 (aq) solution where all SO2 is oxidized to SO2−4. The resulting solution of I2 required 90 ml of 0.1 M Na2S2O3(aq) solution.Calculate rate constant (in hr−1) of the reaction. Given : log 2 = 0.3___
Answer» 0.004 mol of $S O_{2} C l_{2} (g)$ is taken in a sealed vessel where it decomposes as $S O_{2} C l_{2} (g) \to S O_{2} (g) + C l_{2} (g)$ After 0.2303 hours, the gaseous mixture is passed through a 150 $m l$ of acidified, $0.1 N I_{2}$ (aq) solution where all $S O_{2}$ is oxidized to $S O_{4}^{2 -}$ . The resulting solution of $I_{2}$ required 90 $m l$ of 0.1 $M$ $N a_{2} S_{2} O_{3} (a q)$ solution.Calculate rate constant $(i n h r^{- 1})$ of the reaction. Given : log 2 = 0.3___