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Chemical Kinetics

Short Answer Type

131. Identify, giving reasons, the faster reaction in the following:

2 Na (s) + I_{2} (s) \to 2 Nal (s)

2 Na (s) + I_{2} (g) \to 2 Nal (s)

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132. Identify, giving reasons, the faster reaction in the following:

C (s) + 2 H_{2} O (g) \to 2 H_{2} (g) + {CO}_{2} (g)

C (s) + 2 H_{2} O (s) \overset{Catalyst}{\to} 2 H_{2} (g) + {CO}_{2} (g)

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133. Identify, giving reasons, the faster reaction in
the following:

C (s) + 1 / 2 O_{2} (g) \overset{500 °}{\to} CO (g) C (s) + 1 / 2 O_{2} (g) \overset{1000 °}{\to} CO (g)

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134. Identify, giving reasons, the faster reaction in the following:

N_{2} (10 atm) + 3 H_{2} (10 atm) \to 2 {NH}_{3} (g) N_{2} (5 atm) + 3 H_{2} (5 atm) \to 2 {NH}_{3} (g)

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135. What is the difference between order and molecularity of a reaction?

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Long Answer Type

136. What are Pseudo chemical reaction? Give examples.

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Short Answer Type

137. A reaction is first order in A and second order in B.
(i) Write differential rate equation.
(ii) How is the rate affected if the concentration of B is tripled?
(iii) How is the rate affected when the concentrations of both A and B are doubled?
What is the significance of rate constant in the rate expression?

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138. Following reaction takes place in one step:

2 NO (g) + O_{2} (g) ⇋ 2 {NO}_{2} (g)

How will the rate of the above reaction change if the volume of the reaction vessel is diminished to one third of its original volume? Will there be any change in the order of the reaction with the reduced volume ?

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139. Two similar reactions have the same rate constant at 25°C, but at 35°C one of the reaction has a higher rate constant than the other. Account for these observations.

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Long Answer Type

140. How will you verify whether a reaction is first order or not?

Whether a reaction is of first order or not can be verified by using the analytical methods based on the rate equations. The reagents are allowed to react, the change of concentration is measured at different time intervals. For a first order reaction:

(i) Plot of log [A₀]/[A] versus t gives a straight line passing through the origin.

(ii) Plot of log[A] versus t gives a straight line with an intercept log [A]₀ and a slope = – k /2.303.

(iii) Plot of [A] versus t is exponential.

(iv) The value of k calculated by using kt = 2.303 log [A]₀/ [A] for different time intervals come out to
be same.

(v) The half life period is independent of the initial concentration of the reactant.

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