Question

# For each run of the iodine clock reaction, 5.00 mL of a 2.02×10-2 M arsenious acid...

For each run of the iodine clock reaction, 5.00 mL of a 2.02×10-2 M arsenious acid solution is added to the reaction mixture. The total volume of the reaction mixture is 100.0 mL. What is the initial rate of the reaction if the solution turns blue after 68 seconds?

Given information:

• Initial rate of arsenious acid is 2.02 10-2 M
• Time is 68 seconds

The iodine clock reaction is shown below:

The initial rate for arsenious acid at 68 seconds is calculated as follows:

Negative sign only shows the decomposition of arsenious acid. Therefore, the initial rate for arsenious acid at 68 seconds is 9.9 × 10-5 M s-1.

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