Chemistry?

Question

94. The thiosulfate ion (S2O3^(-2))) is oxidized by iodine as follows: 

 

2S2O3^(-2) + I2 ---> S4O6^(-2) +2I^(-)

In a certrain experiment, 7.05 * 10 ^(-3) mol/L of S2O3^(-2) is consumed in the first 11.0 seconds of the reaction. Calculate the rate of consumption of S2O3^(-2). Calculate the rate of production of iodide ion.

 

Answer 1

Step 1:

The chemical equation is .

The concentration of is 7.05 * 10^-3 M.

Time taken to consume is 11.0 sec.

Rate of consumption of is .

Rate of consumption of is .

Step 2:

Rate of production of iodine:

        (since change in concentration of is negligible)

Rate of production of iodine is .

Solution:

Rate of consumption of is .

Rate of production of iodine is .