Thiosulfate ion S2O32− is oxidized by ioidine according to the following reaction. 2S2O32−(aq) + I2(aq) ¨ S4O62−(aq) + 2I−(aq). If in a certain experiment, 0.0020mole of thiosulfate ion is consumed in 1.0 L of solution in 1 second, what is the rate of consumption of iodine. ?

Question

Thiosulfate ion S2O32− is oxidized by ioidine according to the following reaction. 2S2O32−(aq) + I2(aq) ¨ S4O62−(aq) + 2I−(aq). If in a certain experiment, 0.0020mole of thiosulfate ion is consumed in 1.0 L of solution in 1 second, what is the rate of consumption of iodine. ?

DrBob222 · Answer

rate S2O3^2- is 1/2*0.002M/s rate I2 consumption is 0.002 M/s

Thiosulfate ion S2O32− is oxidized by ioidine according to the following reaction. 2S2O32−(aq) + I2(aq) �¨ S4O62−(aq) + 2I−(aq). If in a certain experiment, 0.0020mole of thiosulfate ion is consumed in 1.0 L of solution in 1 second, what is the rate of consumption of iodine. ?