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Chemical Kinetics

Short Answer Type

91. Write the rate of reaction for the following reactions in terms of the concentration of reactants and products
(i) 2H₂O₂→ 2H₂O + O₂(ii) 2NO + O₂ → 2NO₂

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92.

Nitric Oxide. NO reacts with oxygen to produce nitrogen dioxide.
2NO(g) + O₂(g) → 2NO₂(g)
The rate law for this reaction is
rate = k[NO]² [O₂]
Propose a mechanism for the above reaction.

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93. State the role of activated complex in a reaction and state its relation with activation energy?

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94. For the reaction:
2NO(g)+ O₂(g) → 2NO₂(g)
the rate law is
Rate = k[NO]². Why does the rate law not include the concentration of O₂?

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95.

The rate of reaction
2NO + Cl₂ → 2NOCl
is double when concentration of Cl₂ is doubled and it becomes 8 times when concentrations of both NO and Cl₂ are doubled. Deduce the order of this reaction.

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96. Define ‘energy of activation’ of a reaction. How does it vary with a rise in temperature?

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Long Answer Type

97. State and explain Arrehenius equation. How can we determine the activation energy of a reaction using this equation?

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98. What are Photo-chemical reactions? Describe the mechanism of reaction between hydrogen gas and chlorine gas when exposed to sunlight?

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Short Answer Type

99. From the potential energy diagram show that: ΔE = over all energy change for the forward reaction: Ea₁ – Ea₂; where Ea₁ = Activation energy for the forward process and Ea₂ = Activation energy for the reverse process?

Reaction coordinate represents the profile of energy change when reactants change into products.

E_{R} = E_{r} - E_{a_{1}} E_{P} = E_{r} - E_{a_{2}} ∆ E = E_{p} - E_{R} = (E_{r} - E_{a_{2}}) - (E_{r} - E_{a_{1}}) = E_{a_{1}} - E_{a_{2}} .

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100. The form of the rate law for a reaction is expressed as: rate = k [Cl₂] [NO]². Find out the orders of reaction with respect to Cl₂ and with respect to NO and also the overall order of the reaction.

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