Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of ·0.0058Ms−1:→2HIg+H2gI2gSuppose a 3.0L flask is charged under these conditions with 100.mmol of hydrogen iodide. How much is left 1.0s later? You may assume no other reaction is important.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Question
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of ·0.0058Ms−1:→2HIg+H2gI2gSuppose a 3.0L flask is charged under these conditions with 100.mmol of hydrogen iodide. How much is left 1.0s later? You may assume no other reaction is important.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Solution
The rate of a zero order reaction is given by the equation:
[HI] = [HI]₀ - kt
where: [HI] is the final concentration of hydrogen iodide, [HI]₀ is the initial concentration of hydrogen iodide, k is the rate constant, and t is the time.
First, we need to calculate the initial concentration of hydrogen iodide. The concentration is given by the number of moles divided by the volume. So,
[HI]₀ = 100 mmol / 3.0 L = 33.33 mmol/L
Next, we can substitute the known values into the rate equation:
[HI] = 33.33 mmol/L - 0.0058 mmol/L*s * 1.0 s = 33.33 mmol/L - 0.0058 mmol/L = 33.32 mmol/L
So, after 1.0 second, there are approximately 33.32 mmol/L of hydrogen iodide left in the flask.
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