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Chemical Kinetics

Short Answer Type

101. (a)Show graphically how the rate of a first order reaction with only one reactant depends upon the concentration of the reactant.
(b) Give one example of a first order reaction.

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102. A possible mechanism for the reaction

If the second step is the rate determining step, what is the rate law for this reaction?

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103. Express the relationship between the rate of production of water and the rate of disappearance of oxygen in the following reaction:

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

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104. Express the relationship between the rate of production of NOCl and the rate of disappearance of chlorine in the following reaction:

2 NO + {Cl}_{2} \to 2 NOCl .

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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} .

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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?

R_{1} = \frac{dx}{dt} = k {[A_{1}]}^{a} {[B_{1}]}^{b}

...(i)

R_{2} = k [A_{2}]^{a} {[B_{1}]}^{b}

...(ii)

Dividing (ii) by (i), we get

\frac{R_{2}}{R_{1}} = {[\frac{A_{2}}{A_{1}}]}^{a}

From this a can be calculated

R_{3} = k {[A_{1}]}^{a} {[B_{2}]}^{b}

...(iii)

Dividing (iii) by (i)

{(\frac{R_{3}}{R_{1}})}^{1} = {(\frac{B_{2}}{B_{1}})}^{b} T h u s b = 1

From this we can calculate b.

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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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