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Chemical Kinetics

Question

Explain the relationship between the rate of production of iodine and rate of disappearance of hydrogen iodide in the following reaction?
$2 HI \to H_{2} + I_{2} .$

Solution

Rate of disappearance of HI

$= \frac{- d [HI]}{dt}$

Rate of appearance of $I_{2} = \frac{d [I_{2}]}{dt} .$

From the chemical equation,
Rate of production $I_{2}$

$= \frac{1}{2} \times Rate of disappearance of HI$

Therefore, $\frac{d [I_{2}]}{dt} = \frac{1}{2} \frac{d [HI]}{dt} .$

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Chemical Kinetics

Explain the relationship between the rate of production of iodine and rate of disappearance of hydrogen iodide in the following reaction?
$2 HI \to H_{2} + I_{2} .$

Some More Questions From Chemical Kinetics Chapter

What will be the effect of temperature on rate constant?

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction.

The rate law for the decomposition of N₂O₅ is rate = k[N₂O₅]. What is the significance of k in this equation?

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For Daily Free Study Material Join wiredfaculty

Chemical Kinetics

Explain the relationship between the rate of production of iodine and rate of disappearance of hydrogen iodide in the following reaction? 2HI → H2+I2.

Some More Questions From Chemical Kinetics Chapter

What will be the effect of temperature on rate constant?

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction.

The rate law for the decomposition of N2O5 is rate = k[N2O5]. What is the significance of k in this equation?

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

Explain the relationship between the rate of production of iodine and rate of disappearance of hydrogen iodide in the following reaction?
$2 HI \to H_{2} + I_{2} .$

The rate law for the decomposition of N₂O₅ is rate = k[N₂O₅]. What is the significance of k in this equation?