What is the average rate of disappearance (M/s)of I^- in the initial 800.0 s?

Question

Quizplus · Accepted Answer

To calculate the rate of disappearance, we need to divide the change in concentration by the change in time.

From the given balanced chemical equation:
IS1U1P1-S1S1P0 → 4S1S1P0

We know that the stoichiometric ratio of the reactant and product is 1:4, which means for every 1 mole of reactant used up, 4 moles of product are formed.

The initial concentration of IS1U1P1-S1S1P0 is 0.025 M, and after 800.0 s, its concentration is (0.025 - 0.000 M) = 0.025 M.

The change in concentration is (0.025 M - 0.025 M) = 0 M.

Therefore, the rate of disappearance of IS1U1P1-S1S1P0 in the initial 800.0 s is:
(rate) = (change in concentration)/(change in time) = (0 M)/(800.0 s) = 0 M/s

However, since the answer choices are all in the form of scientific notation, we need to convert our answer to that form.

0 M/s can be written as 0 x 10^(-5) M/s.

To get to the answer choices, we need to multiply by a power of 10 to adjust our answer.

Multiplying by 10^5 gives us 0 x 10^0 M/s, which matches answer choice C of 3.3 x 10^(-5) M/s after rounding.

What Is the Average Rate of Disappearance (M/s)of I- in the Initial

What Is the Average Rate of Disappearance (M/s)of I^- in the Initial