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

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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106. Explain the relationship between the rate of production of oxygen and the rate of disappearance of hydrogen peroxide (H₂O₂) in the following reaction:

2 H_{2} O_{2} \to 2 H_{2} O + O_{2}

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107. Starting with differential rate law equation for a first order reaction, derive the integrated rate law equation for a first order reaction. How is it related to the rate constant?

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108. What is the initial rate method for the determination of a reaction rate when more than one reactant is present?

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109. For the reaction:

3 H_{2} (g) + N_{2} (g) \to 2 {NH}_{3} (g)

express the rate of the reaction in terms of

- d [H_{2}] / dt, - d [N_{2}] / dt and d [{NH}_{3}] dt .

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110. For the reaction:
NO₂(g) + CO (g) → CO₂(g) + NO(g)
the experimentally determined rate expression between 440 K is rate = k[NO₂]². What mechanism can be proposed for the above reaction?

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