A constant current was flown for 2 hour through a solution of KI. At the end of experiment liberated lodlne consumed 21.75 mL of 0.0831 M solution of sodium thiosulphate followihg the reaction: `I_(2)+2S_(2)O_(3)^(2-) to 2I^(-) +S_(4)O_(6)^(2-)`. What was the aveagre rate of current flow in ampere?

Explanation

To solve the problem step by step, we will follow the given information and apply the relevant concepts from electrochemistry.

### Step 1: Calculate the moles of iodine (I2) produced
We know that the volume of sodium thiosulphate (Na2S2O3) used is 21.75 mL and its molarity is 0.0831 M.

First, convert the volume from mL to L:
\[
\text{Volume (L)} = \frac{21.75 \text{ mL}}{1000} = 0.02175 \text{ L}
...